1. State whether the H2O in each of the following chemical equations is acting a

ID: 829948 • Letter: 1

Question

1. State whether the H2O in each of the following chemical equations is acting as an acid or a base.

2. Write a balanced equation for each of the following neutralization reactions. If needed, refer to your text for help with formulas.

a. Ammonium hydroxide with hydrobromic acid

b. Acetic acid with lithium hydroxide

c. Sulfuric acid with potassium hydroxide

d. Nitric acid with sodium hydroxide

3. What volume of concentrated hydrochloric acid (12 M HCl) will be needed to prepare 500 mL of .10 M HCl?

4. How many grams of potassium hydrogen phthalate (KHP) will be required to completely neutralize 50 mL of .15 M NaOH solution?

1. (a) C2H5SH + H2O => C2H5S- + H3O+

Since H2O accepts a proton => base

(b) CH3COOH + H2O => CH3COO- + H3O+

Since H2O accepts a proton => base

Since H2O donates a proton => acid

(d) CH3CH2NH2 + H2O => CH3CH2NH3+ + OH-

Since H2O donates a proton => acid

2. (a) NH4OH(aq) + HBr(aq) => NH4Br(aq) + H2O(l)

(b) HC2H3O2(aq) + LiOH(aq) => LiC2H3O2(aq) + H2O(l)

(d) HNO3(aq) + NaOH(aq) => NaNO3(aq) + H2O(l)

3. M1V1 = M2V2

12 x V1 = 0.10 x 500

Volume V1 = 4.17 mL (approximately 4.2 mL)

4. KHP + NaOH => NaKP + H2O

Moles of KHP = moles of NaOH = volume x concentration of NaOH

= 50/1000 x 0.15 = 0.0075 mol

Mass of KHP = moles x molar mass of KHP

= 0.0075 x 204.22 = 1.53 g (approximately 1.5 g)

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