NaOH was standardized by titration against a standard acidic solution of potassium hydrogen phthalate (abbreviated KHP). NaOH reacts with KHP in a ratio of 1:1. 0.750 g of KHP were dissolved in 100 ml of water to prepare the standard KHP solution. a. KHP has the chemical formula C8H5KO4. Calculate its molar mass from the periodic table. b. If 25.22 ml of sodium hydroxide were required to neutralize the above preparec KHP standard solution, what is the molarity of NaOH? (Hint: first calculate the molarity of KHP standard solution). Show all your calculations.

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s) 0.250 g of HI is dissolved in 300. mL of a 0.00520 M solution of Ca(OH)2. (Assume this does not change the volume). The dissolved salts then proceed to react. a. What is the balanced chemical reaction (include states)? b. What type of reaction is this? С. What is the limiting reactant? d. How many grams of water are produced from this reaction?

6. Sodium sulfide reacts with hydrochloric acid to produce hydrogen sulfide and sodium chloride. How many grams of sodium sulfide are required for complete reaction with 15.0 mL of 0.250 M hydrochloric acid? The molar mass of sodium sulfide is 78.046 g/mol. (Hint: start by writing the balanced equation for the reaction.)

8. A student adds 22.36 mL of 1.366 x 10¹ M Mg(OH), in order to completely neutralize 25.00 mL of H₂PO acid. Calculate the original concentration of the acid solution.

a. Calculate the molarity of a solution that contains 0.175 mol ZnCI2 in exactly 150 mL solution. b. How many milliliters of a 6.00 M NaOH solution are needed to provide 0.350 mol of NaOH?

4. When a solutions of aluminum sulfate and potassium hydroxide are mixed, a precipitate forms. a. Write a balanced net ionic equation for the reaction. b. Calculate the mass of the precipitate when 3.89 g of aluminum sulfate in 100mL of solution is combined with 50 mL of the o.300 M KOH. c. What is the molarity of the ion in excess? (Ignore the spectator ions and assume that volumes are additive)

In an experiment, a student combines 75.0 mL of a 0.190 M iron (III) chloride solution with 125.0 mL of a 0.240 M sodium carbonate solution. a. Write a balanced equation for the reaction to see how many grams of sodium chloride need to be produced in the experiment in order to achieve a yield of 83.75%?

3. Nitric acid reacts with potassium hydroxide. a. Write a balanced chemical equation to describe this reaction b. 50.0 mL of a nitric acid solution is titrated with 48.6 mL of 0.124 M potassium hydroxide solution. i. Calculate the moles of potassium hydroxide used for the titration. 50.0mL ii. Calculate the molarity of the 50mL nitric acid solution before the reaction.

2. Acetic acid (HC2H3O2) is an important component of vinegar. A 10.0-mL sample of vinegar is titrated with 0.255 M NAOH, and 13.5 mL are required to neutralize the acetic acid that is present. a. Write a balanced equation for this neutralization reaction. b. What is the molarity of the acetic acid in this vinegar? c.lf the density of the vinegar is 1.006 g/mL, what is the mass percent of acetic acid in the vinegar?