Question

1. What is the pH of the following solutions? 0.65M HNO3 0.0205 M Ba(OH)2 3.Calculate the [OH -] for the solutions with a pH of 10.82. Is the solution acidic, basic, or neutral? 4. A student is to dissolve 8.75g of Sr(OH)2 in enough water to get a pH of 13.35. What should the final volume be? 5.Which of the following is the strongest acid? Acid pOH HA 8.71 HB 9.21 HC 3.17 HD 4.29 HE 7.00 6. Label each species in the equations below as acids or bases and connect the conjugate pairs. CO2 + H2O  H3O+ + HCO3- H2SO4 + H2PO4-2  HSO4- + H3PO4 7. Classify the following as acidic, basic, or neutral. pH = 6.0 [H+] = 1 X 10-8 M pOH = 4.5 [OH-] = 1 X 10-8 M pH = 7.0 8. In a titration, a sample of H2SO4 solution with a volume of 15.00 mL required 36.42 mL of 0.147 M NaOH for complete reaction. What is the molarity of the H2SO4 solution?

Answer 1

1. 0.65 M HNO₃

2. 0.0205 M Ba(OH)₂

3.

Solution is basic in nature since pH is more than 7.

4.

5. Less the pH, more will be acidic nature. Hence, Acid with highest pOH will be most acidic.

HB is the strongest acid.

7. pH = 6 - Acidic

[H⁺] = 10^-8 M - Basic

pOH = 4.5 - Basic

[OH^-] = 10^-8 - Acidic

pH = 7 - Neutral

8. Milimoles of NaOH = 0.147 x 36.42

Milimoles of NaOH = 5.35374

Milimoles of H₂SO₄ = 5.35374 / 2 = 2.67687

Volume of H₂SO₄ = 15 mL

Molarity of H₂SO₄ = 2.67687 / 15

Molarity of H₂SO₄ = 0.178 M