XC-10 Due at the time of SA 1. Which of the following substances is a base when dissolved in water, as defined by Arrhenius? magnesium sulfate magnesium.

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XC-10 Due at the time of SA 1. Which of the following substances is a base when dissolved in water, as defined by Arrhenius? magnesium sulfate magnesium hydroxide magnesium chloride magnesium acetate 2. In each of the following equations, identify the reactant that is a Brønsted–Lowry acid and the reactant that is a Brønsted–Lowry base: 3. Which of the following sets of chemicals is an acid-base conjugate pair? HClO2(aq) & ClO2 ¯(aq) H2O(aq) & HClO2(aq) H3O+(aq) & ClO2 ¯(aq) HClO2(aq) & ClO¯(aq) 4. Write the formula of the conjugate base of each of the following Brønsted–Lowry acids: HClO3 H2CO3 5. Identify the conjugate acid–base pairs in the following equation:

7. What is the [H3O+] of a solution if [OH−] is 5.0 x 10-8 M? 6. A vinegar solution has a [H3O+] = 2.0 x 10–3 M at 25 °C. What is the [OH–] of the vinegar solution? Is the solution acidic, basic, or neutral? 7. What is the [H3O+] of a solution if [OH−] is 5.0 x 10-8 M? 8. Given that the pH of a solution is 6.7, what is the [H3O+]? 5.0 × 106 M 8.0 × 10-1 M 1.9953 × 10-7 M 2.0 × 10-7 M

10.8 9. Determine the pH for the following solutions: [H3O+] = 1.0 x 10–5 M [H3O+] = 5 x 10–8 M 10.8 10. A solution has a pH of 8.5. What is the molarity of hydrogen ions in the solution? 11. What is the pH of an ammonia solution at 25 ˚C with [OH–] = 3.7 x 10–3 M?

12. Use the given table to select the acid that fits the following criteria: weak acid stronger than HF(aq). HCl(aq) H3PO4(aq) HNO3(aq) H2CO3(aq) 13. Which of the following pairs would make a buffer solution? HF(aq) and NaCl(aq) HCN(aq) and NaCN(aq) HBr(aq) and NaCl(aq) HCl(aq) and LiOH(aq) 14. The acid-base pair in a buffer is H2PO4– /HPO42–, which has a Ka of 6.2 x 10–8. What is the pH of a buffer that is 0.10 M H2PO4– and 0.50 M HPO42–?