Questions!

Question 1:

Q: A neutralization reaction has two products _______ and _________.
A: Salt, water

Question 2:

Q: A solution has an H+ concentration of 0.0001. Is it an acid, a base, or neutral? What is the pH?
A: Acid. 4.

Question 3:

Q: A solution has an OH- concentration of 1 x 10-8 Is it an acid base or neutral? What is the pOH?
A: Base. 8.

Question 4:

Q: A solution of Ca(OH)2 is 5.4 x 10-6 M. What is the pH?
A: The pH is 9.03

Question 5:

Q: A solution of H2SO4 is 0.025M. What is the pH?
A: The pH is 1.3

Question 6:

Q: A solution of HCl is 0.0034 M. What is the pH?
A: The pH is 2.46

Question 7:

Q: Acids are frequently found in _____________.
A: food

Question 8:

Q: Acids could have a pH of?
A: 0 - 6.9

Question 9:

Q: Bases are often found in ____________.
A: Cleaning products

Question 10:

Q: Bleach is an example of a(n) ?
A: Base.

Question 11:

Q: Free H+ will associate with H2O, which forms?(Formula and name)
A: H3O+ Hydronium.

Question 12:

Q: H2S is named?
A: Hydrosulfuric acid

Question 13:

Q: H2SO4 is named?
A: Sulfuric acid

Question 14:

Q: HNO2 is named?
A: Nitrous acid

Question 15:

Q: How do acids taste?
A: Sour

Question 16:

Q: How do bases feel when you touch them?
A: Slippery

Question 17:

Q: How do bases taste?
A: Bitter

Question 18:

Q: Hydrobromic acid's formula is?
A: HBr

Question 19:

Q: Mixing an acid and a base together results in a _______________ reaction.
A: Neutralization

Question 20:

Q: NH3 is a ?
A: Base

Question 21:

Q: OH- is called?
A: Hydroxide

Question 22:

Q: pH 3 has an H+ concentration of?
A: 1 x 10-3 M

Question 23:

Q: pH 4 is equal to pOH ?
A: pOH 10

Question 24:

Q: pH 7 is known as?
A: Neutral

Question 25:

Q: Phosphoric acid's formula is?
A: H3PO4

Question 26:

Q: pOH 13 is equal to pH?
A: pH 1

Question 27:

Q: pOH 6 has an OH- concentration of?
A: 1 x 10-6 M

Question 28:

Q: Solutions are acidic if they have a larger concentration of?
A: H+ ions

Question 29:

Q: Solutions are basic if the have a larger concentration of?
A: OH- Hydroxide ions

Question 30:

Q: Strong acids would have a pH of ?
A: 0 or 1

Question 31:

Q: The pH scale includes number between ?
A: 0 to 14

Question 32:

Q: This scale measures the concentration of hydroxide?
A: pOH

Question 33:

Q: To what color do acids turn Litmus paper?
A: Red

Question 34:

Q: To what color do bases turn Litmus paper?
A: Blue

Question 35:

Q: Water, acids and bases all break apart to some degree. What is this called ?
A: Dissociation

Question 36:

Q: Weak acids would have a pH of?
A: pH 6

Question 37:

Q: Weak bases would have a pH of?
A: pH 8

Question 38:

Q: What are the three rules for naming acids?
A: -ide --> add Hydro and ic. -ate --> add ic. -ite --> add ous

Question 39:

Q: What does Arrhenius' theory of acids and bases state?
A: Acids dissociate H+. Bases dissociate OH-

Question 40:

Q: What does the Bronsted-Lowry theory of acids and bases state?
A: Acids donate H+. Bases accept H+.

Question 41:

Q: What is the difference between strong and weak acids and bases?
A: The amount of dissociation. Strong acids and bases dissociate almost 100%

Question 42:

Q: What is the name of the acid and base testing papers?
A: Litmus paper

Question 43:

Q: What is the name of the scale that measures acidity or basicity?
A: The pH scale

Question 44:

Q: What is the pH of salt (NaCl) water?
A: pH 7

Question 45:

Q: When testing something with Litmus paper, what result would tell you the solution is neutral?
A: Neither the red nor the blue papers change color.

Question 46:

Q: Who came up with the original definition of acids and bases?
A: Svante Arrhenius

Question 47:

Q: Who said that NH3 is a base because it accepts H+ ions?
A: Johannes Bronsted and Thomas Lowry.

Question 48:

Q: Why do strong acids conduct electricity better than weak acids?
A: Because there are a larger number of dissociated H+ ions that can move through the solution.

Question 49:

Q: Why is NH3 a base?
A: Because it accepts H+ ions and thus increases the amount of OH- compared to H+

Question 50:

Q: Why is pH 7 neutral?
A: Because the amounts of H+ and OH- are equal.

Question 51:

Q: Who is the really vampirey looking scientist?
A: Johannes Bronsted

Question 52:

Q: What is the name for H2CO3?
A: Carbonic Acid

Question 1:

Q: This represents the point on a phase diagram where temperature and pressure of all 3 phases of matter of a substance coexist.
A: The triple point

Question 2:

Q: If the temperature of 34.4 g of ethanol increases from 25.0 degrees Celsius to 78.8 degrees Celsius, how much heat has been absorbed by the ethanol? (Specific heat of ethanol is 2.44)
A: 4515.8 J

Question 3:

Q: The symbol letter for specific heat is? Include unit!
A: c

Question 4:

Q: The specific heat of liquid water is ?
A: 4.184 J/g degrees C

Question 5:

Q: A change in temperature is found by doing what? Be specific.
A: Subtracting End - Start temperatures

Question 6:

Q: A chocolate bar contains 142 nutritional Calories. Convert this energy to calories.
A: 142000 calories

Question 7:

Q: In an exothermic reaction, energy is __________.
A: released

Question 8:

Q: What information is located on the Y axis in a phase diagram?
A: Pressure

Question 9:

Q: One Calorie is equal to ___ kcals.
A: 1

Question 10:

Q: The symbol letter for heat is _____.
A: Q

Question 11:

Q: Energy that is in motion is called _______ ______.
A: Kinetic Energy

Question 12:

Q: What information is located on the X axis in a phase diagram?
A: Temperature

Question 13:

Q: What are the 2 units of measurement for energy?
A: Joules and calories

Question 14:

Q: Energy that is due to the composition or position of an object is called ______ _________.
A: Potential energy

Question 15:

Q: The amount of heat required to raise the temperature of one gram of a substance by one degree Celsius is called _________ ______.
A: Specific Heat

Question 16:

Q: In an endothermic reaction, energy is __________.
A: absorbed

Question 17:

Q: What can you conclude about a swimming pool that is cold in the morning?
A: It lost energy during the cold night.

Question 18:

Q: The heat content of a system, or energy inside is called its __________
A: Enthalpy

Question 19:

Q: The symbol letter for enthalpy is
A: H

Question 20:

Q: Exothermic reactions have a _________ delta H
A: Negative

Question 21:

Q: Endothermic reaction have a __________ delta H
A: Positive

Question 22:

Q: Na(s) + H2O(l) --> NaOH(aq) + H2(g) + 75kJ is a thermochemical equation. This reaction is ______thermic
A: Exo

Question 23:

Q: Freezing water is an ________thermic process.
A: Exo

Question 24:

Q: CO2(s) --> CO2(g) This process is called ___________ and is an ______thermic process.
A: Sublimation, Endo

Question 25:

Q: CO2(g) --> CO2(s) This process is called ___________ and is an ______thermic process.
A: Deposition, Exo

Question 26:

Q: Vaporizing water is an _____thermic process
A: Endo

Question 27:

Q: Changing from liquid to gas is called ________ and is an ____thermic process
A: Condensation, Exo

Question 28:

Q: 350 g of water is cooled from 85 degrees Centigrade to 15 degrees Centigrade. What is the energy change for this process?
A: Negative 102508 J

Question 29:

Q: You use 50000 J to heat water from 10 to 17 degrees Celsius. How many grams of water are you heating?
A: 1707.2 grams

Question 30:

Q: This is the amount of disorder in a system.
A: Entropy

Question 31:

Q: This is the average energy in the system.
A: Temperature

Question 32:

Q: This type of energy is the total energy that molecules have in their movement.
A: Heat

Question 33:

Q: This is the ability to do work or make heat.
A: Energy

Question 34:

Q: Which has more total heat, a giant piece of ice or one drop of boiling water?
A: Giant piece of ice

Question 35:

Q: Which has a higher temperature, a giant piece of ice, or one drop of boiling water?
A: One drop of boiling water

Question 36:

Q: What is the name of the cup + thermometer that we used to measure the energy given from the hot metal to the cool water?
A: A calorimeter

Question 37:

Q: The _______________________________ states that energy cannot be created or destroyed, only changed from one kind to another.
A: Law of Conservation of Energy

Question 38:

Q: In the lab, why did the temperature of the water only change a little, but the temperature of the metal change a lot?
A: Because the specific heat of the water is much higher than that of the metal.

Question 39:

Q: The phase of a material is affected by two things, temperature and ________
A: Pressure

Question 40:

Q: The __________ ______ in a phase diagram is the point at which the line between gases and liquids stops.
A: Critical Point

Question 41:

Q: In an _____thermic process, the products contain more energy than the reactants.
A: Endo

Question 42:

Q: In an _____thermic process, the reactants contain more energy than the products.
A: Exo

Question 43:

Q: A beaker containing a reaction becomes cold. The reaction is _____thermic
A: Endo

Question 44:

Q: H2 + O2 --> H2O + 200 J is an _____thermic reaction
A: Exo

Question 45:

Q: A catalyst is used for what purpose?
A: To decrease the activation energy and speed up a reaction

Question 46:

Q: ________ energy is the energy rquired to begin a reaction.
A: Activation

Question 47:

Q: A graph of energy versus time with a negative slope is an ____thermic graph
A: Exo

Question 48:

Q: A graph of energy versus time with a positive slope is an ____thermic graph
A: Endo

Question 49:

Q: A graph of energy versus time that goes up is an ____ thermic graph
A: Endo

Question 50:

Q: A graph of energy versus time that goes down is an ____ thermic graph
A: Exo

Question 51:

Q: On a heating curve, temperature of a substance is plotted on the y axis. During what two parts is the line flat?
A: During melting and vaporization the line is flat.

Question 52:

Q: Photosynthesis is an ____thermic process that takes light energy and converts it into ________ ________ energy. (extra point!)
A: Endo, Chemical potential

Question 53:

Q: A bag of cookies contains 15 cookies. You read on the label that one serving is 3 cookies. Each serving contains 130 Calories. How many Calories are in the whole bag?
A: 650 Calories

Question 54:

Q: How many calories are there in 120 Calories?
A: 120000 calories

Question 55:

Q: A rock precariously balanced on the edge of a cliff has a lot of ________ energy that may soon turn into _______ energy as it falls.
A: Potential energy, kinetic energy

Question 56:

Q: The type of energy contained in sugar is called chemical potential energy. Where, precisely, is this energy located?
A: In the bonds.

Question 1:

Q: Balance this reaction, write the mole ratio and name its type. KClO3 --> KCl + O2
A: 2:2:3 decomposition

Question 2:

Q: What are the five types of reactions?
A: Single Displacement, Double Displacement, Combustion, Decomposition, Synthesis

Question 3:

Q: How many particles are in 2 moles?
A: 1.2044 x 10^24 particles

Question 4:

Q: How many particles are in 10 grams of Carbon?
A: 5.01 x 10^23 particles of Carbon

Question 5:

Q: What is a limiting reactant?
A: The reactant that is used up first

Question 6:

Q: What is the opposite of the limiting reactant called?
A: The excess reactant.

Question 7:

Q: What does stoichiometry study?
A: The amounts of products and reactants in a reaction.

Question 8:

Q: For the reaction NaBr + Cl2 --> NaCl + Br2 what would the limiting reactant be if 10 moles of NaI was combined with 6 moles of Cl2?
A: The NaBr

Question 9:

Q: Why do equations have to be balanced?
A: To obey the law of conservation of mass: no matter can ever be created or destroyed

Question 10:

Q: What is the percent composition of oxygen in H2SO4?
A: 65.2% Oxygen

Question 11:

Q: You work a limiting reactant problem, and get two answers for the amount of product: 10 g and 8 g. Which is the correct answer?
A: 8 grams

Question 12:

Q: What is a solvent?
A: The substance that causes dissolving

Question 13:

Q: Which solvent is called the universal solvent?
A: Water

Question 14:

Q: An unknown mixture is observed, and no particles are observed to fall to the bottom. How can we tell if this mixture is a solution or a colloid? What result would tell us that the mixture is a colloid?
A: Test for the Tyndall Effect. If a light is observed shining inside the mixture, it is a colloid.

Question 15:

Q: Which type of mixture has large sized particles that sink to the bottom?
A: A suspension

Question 16:

Q: What will happen to a saturated solution that is cooled down?
A: It will become supersaturated, and crystals will fall to the bottom.

Question 17:

Q: How can you make a supersaturated solution?
A: Make a warm saturated solution, and carefully cool it down.

Question 18:

Q: Henry's law describes the relationship between what two things? What is the formula?
A: The pressure, and the solubility of a gas in a liquid. S1/P1 = S2/P2

Question 19:

Q: What happens to the solubility of gases in water as the temperature of the water increases?
A: The solubility of the gas decreases. Poor fishies!

Question 20:

Q: What happens to the solubility of solids in water as the temperature of the water increases?
A: The solubility of the solid increases. Mmm sugary hot coffee!

Question 50:

Q: What is the molar mass of HNO3?
A: 63 g/mol

Question 51:

Q: One mole can also be called ______'s number
A: Avogadro's

Question 52:

Q: If you have 15 g of water, how many moles of water do you have?
A: 0.83 mol

Question 53:

Q: 23 mol H2SO4 is equal to how many grams of H2SO4?
A: 2256.3 grams H2SO4

Question 54:

Q: How many particles are in 25 g of Carbon?
A: 1.25 x 10^ 24 particles of Carbon

Question 55:

Q: What is the difference between an empirical and a molecular formula?
A: A molecular formula contains the real number of atoms, while an empirical formula is a reduced formula found by experiment.

Question 56:

Q: What is the empirical formula for C45H15O6?
A: C15H5O2

Question 57:

Q: What are the steps for solving an empirical formula problem?
A: Pretend % are grams, find moles by dividing each by molar mass, divide by smallest number, place numbers in correct spots.

Question 58:

Q: What’s the empirical formula of a molecule containing 65.5% carbon, 5.5% hydrogen, and 29.0% oxygen?
A: C3H3O

Question 59:

Q: If the empirical formula of an organic compound is found to be C2H4, and the molar mass is found to be 112 g, what is the molecular formula?
A: C8H16

Question 60:

Q: What does the Tyndall Effect look like, and which types of mixtures will have a positive and which a negative result?
A: The Tyndall Effect is seen as a visible light inside a mixture – either a colloid or a suspension will show a positive Tyndall Effect, whereas a solution will have a negative result

Question 61:

Q: Where would you find points representing unsaturated, saturated and supersaturated mixtures on a solubility curve?
A: Under, On and Above the line

Question 62:

Q: An 80 degree C solution of NaBr holds 65 g in 100 g H2O. If the solution is cooled to 50 degrees C, which has a solubility of only 25 g, what will happen?
A: A supersaturated solution will form, which will eventually precipitate 40 g of crystals.

Question 63:

Q: You have a 2M solution of HCl. You want to make 500 mL of a 0.8 M solution. How much 2M do you need to use? How much water should you add?
A: 200 mL , 300 mL

Question 64:

Q: You are still an infamous international spy. You have a concentrated solution of 5 M As2O5, which is a powerful poison. You need to prepare 0.08 L of 0.02 M As2O5 for the assassination of your enemies' boy scout troop How much of the concentrated solution will you need?
A: 0.00032L

Question 65:

Q: What is the molarity of a sodium chloride solution which contains 5 mols in 3 Liters of water?
A: 1.67 M

Question 66:

Q: What is the molarity of a sodium chloride solution which contains 65 g in 2000 mL of water?
A: 0.56 M

Question 67:

Q: Give an example of a solution, and name which part is the solute and which the solvent.
A: Ex: Salt water: salt is solute, water is solvent

Question 68:

Q: Water and oil do not mix because water is polar and oil is non polar. What is the term for two liquids which cannot mix?
A: Immiscible

Question 69:

Q: Soap is useful due to its ability to make water and oil ___________, which means that the two liquids are able to mix together.
A: Miscible

Question 70:

Q: What is the difference between Bronsted Lowry's definition of bases and Arrhenius' definition of bases?
A: B-L says that bases accept H+, while Arrhenius says that bases donate OH-

Question 1:

Q: Who are you?
A: Elvis!

Question 2:

Q: How many moles are in 300 g of CaCO3?
A: 3.00 mol CaCO3

Question 3:

Q: What is the percent mass of Hydrogen in C6H12O6?
A: 6.7%

Question 4:

Q: If a closed 1.5 L plastic bag containing gas at STP is heated to 300 K, what is the new volume of the bag?
A: 1.65 L

Question 5:

Q: If a closed 1.5 L plastic bag containing gas at STP is pressurized to 150 kPa, what is the new volume of the bag?
A: 1.013 L

Question 6:

Q: 15 mL of juice is mixed with 100 mL of water. What is the percent concentration by volume?
A: 13.04%

Question 7:

Q: 25 g of sugar is dissolved in water, making 300 g of total solution, what is the % concentration by mass?
A: 8.3%

Question 8:

Q: How many atoms of hydrogen does hexane have?
A: 14

Question 9:

Q: How many Carbons does heptane have?
A: 7

Question 10:

Q: What is the name of C9H20?
A: Nonane

Question 11:

Q: What is the new volume of a 2L balloon if the initial pressure is 2 atm, and the pressure is changed to 5 atm?
A: 0.8 L

Question 12:

Q: What temperature in K is equal to -150 Celsius?
A: 123 K

Question 13:

Q: What is the mole ratio found when this equation is balanced? HCl + Mg(OH) 2 --> MgCl2 + H2O
A: 2:1:1:2

Question 14:

Q: HCl + Mg(OH) 2 --> MgCl2 + H2O Using the equation above, if you react 4 moles HCl with 3 moles Mg(OH) 2, which reactant is limiting, and how many moles of MgCl2 can be made?
A: HCl is limiting and 2 moles of MgCl2 can be made

Question 15:

Q: HCl + Mg(OH) 2 --> MgCl2 + H2O Using the equation above, if you begin with 50 g HCl, how many grams of MgCl2 will be produced?
A: 65.3 g MgCl2

Question 16:

Q: HCl + Mg(OH) 2 --> MgCl2 + H2O Using the equation above, if you began with 14 moles of HCl, how many moles of water would be made?
A: 14 moles of water

Question 17:

Q: 2HCl + Mg(OH) 2 --> MgCl2 + 2H2O Using the reaction above, if you begin with 35 g of HCl and 35 g of Mg(OH)2 how many grams of water are actually produced?
A: 17.2 g water

Question 18:

Q: What is standard temperature in C and in K? What is standard pressure in atm and in kPa?
A: 0 degrees Celsius, 273 degrees Kelvin. 1 atm and 101.3 kPa

Question 19:

Q: If 15 g of water is heated from 30 Celsius to 47 Celsius how many calories are used? (The specific heat of water for calories is 1 c/g * C) How many Joules are used? (The specific heat of water for JOULES is 4.184 J/g*C)
A: 255 calories. 1066.92 Joules

Question 20:

Q: A 300 Calorie bite of Snickers bar is burned under a beaker of water. The water is heated from 22 Celsius to 92 Celsius, how many grams of water are in the beaker? (Notice calories and Calories!) (The specific heat of water for calories is 1 c/g*C)
A: 4285.7 grams of water are in the beaker.

Question 21:

Q: One mole of any gas at STP has a volume of 22.4 L ( That is an equality!) . If you have 50 L of O2 at STP, how many moles of gas do you have?
A: 2.23 moles of oxygen gas.

Question 22:

Q: For a neutralization reaction of NaOH and HCl, you expect to make 15 g of salt. However, after you evaporate all the water, you find that you only have 12.3 g of salt. What is your percent yield?
A: 82% yield

Question 23:

Q: How many moles are in 550 g of Ca3(PO4)2?
A: 1.77 mol of Ca3(PO4)2

Question 24:

Q: 15 grams of C6H12O6 is in a solution totaling 400 mL. What is the molar concentration of the solution?
A: 0.21 M
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