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Calculate the concentration of all ions present in each of the following solutions of strong electrolytes.

c. 5.00 g of NH 4Cl in 500.0 mL of solution

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Calculate the concentration of all ions present in each of the following solutions of strong electrolytes.

b. 2.5 mol of Na 2SO4 in 1.25 L of solution

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Calculate the concentration of all ions present in each of the following solutions of strong electrolytes.

a. 0.100 mol of Ca(NO3)2 in 100.0 mL of solution

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A solution of ethanol (C2H5OH) in water is prepared by dissolving 75.0 mL of ethanol (density = 0.79 g/cm3) in enough water to make 250.0 mL of solution. What is the molarity of the ethanol in this solution?

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Calculate the molarity of each of these solutions.

c. A 0.1025-g sample of copper metal is dissolved in 35 mL of concentrated HNO 3 to form Cu2+ ions and then water is added to make a total volume of 200.0 mL. (Calculate the molarity of Cu2+.)

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Calculate the molarity of each of these solutions. 

b. A 184.6-mg sample of K 2Cr2O7 is dissolved in enough water to make 500.0 mL of solution.

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Show how each of the following strong electrolytes “breaks up” into its component ions upon dissolving in water by drawing molecular-level pictures.

a. NaBr

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Differentiate between the following terms.
c. oxidation state versus actual charge

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Differentiate between the following terms.
b. species oxidized versus the oxidizing agent

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Differentiate between the following terms.

a. species reduced versus the reducing agent

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What is an acid and what is a base? An acid–base reaction is sometimes called a proton-transfer reaction. Explain.

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When 1.0 mol of solid lead nitrate is added to 2.0 mol of aqueous potassium iodide, a yellow precipitate forms. After the precipitate settles to the bottom, does the solution above the precipitate conduct electricity? Explain. Write the complete ionic equation to help you answer this question.

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Which of the following statements is(are) true? For the false statements, correct them.

d. All ionic compounds are strong electrolytes in water.

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Which of the following statements is(are) true? For the false statements, correct them.

c. An acid is a strong electrolyte.

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Which of the following statements is(are) true? For the false statements, correct them.

b. A strong electrolyte will break up into ions when dissolved in water.

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Which of the following statements is(are) true? For the false statements, correct them.

a. A concentrated solution in water will always contain a strong or weak electrolyte.

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Differentiate between what happens when the following are dissolved in water.

d. HNO3 versus CO

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Differentiate between what happens when the following are dissolved in water.

c. RbCl versus AgCl

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Differentiate between what happens when the following are dissolved in water.

b. KF versus C 6H12O6

 

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Differentiate between what happens when the following are dissolved in water.

a. polar solute versus nonpolar solute

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Consider separate aqueous solutions of HCl and H 2SO4 with the same molar concentrations. You wish to neutralize an aqueous solution of NaOH. For which acid solution would you need to add more volume (in milliliters) to neutralize the base?
a. the HCl solution
b. the H2SO4 solution
c. You need to know the acid concentrations to answer this question.
d. You need to know the volume and concentration of the NaOH solution to answer this question.
e. c and d
Explain.

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Order the following molecules from lowest to highest oxidation state of the nitrogen atom: HNO3, NH4Cl, N2O, NO2, NaNO2.

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For the reactions in Exercise 38, write the balanced formula equation, complete ionic equation, and net ionic equation. If no precipitate forms, write “No reaction.”

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Natural rubidium has the average mass of 85.4678 and is composed of isotopes 85Rb (mass = 84.9117) and 87Rb. The ratio of atoms 85Rb/87Rb in natural rubidium is 2.591. Calculate the mass of 87Rb.

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You have a solution of table salt in water. What happens to the salt concentration (increases, decreases, or stays the same) as the solution boils? Draw pictures to explain your answer.

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