Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- 1. the temperature for each solution is carried out at approximately 297 K where Kw = 1.00 x 10 ^-14 (a) 0.20 g of hydrogen chloride (HCl) is dissolved in water to make 4.5 L of solution. What is the pH of the resulting hydrochloric acid solution? (b) 0.70 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 3.0 L of solution. What is the pH of this solution ?arrow_forwardA solution is prepared at 25 °C that is initially 0.051M in benzoic acid (HC,H,CO,), a weak acid with K,=6.3 × 10 °, and 0.079M in potassium benzoate (KC,H,CO,). Calculate the pH of the solution. Round your answer to 2 decimal places. pH = [|arrow_forward9 (a) Define and write the expression of Kw for the dissociation of water (H2O). Kw is the of Kw = (b) Calculate the pH of 0.1mol dm-³ potassium hydroxide (KOH(@A) pH =arrow_forward
- Calculate the pH of a solution containing 0.45 M HCN(aq) and 0.65 M NaCN. The Ka of HCN(aq) is 4.9 × 10–10.arrow_forwardculate the pH of a buffer solution 1) Calculate the pH of a solution prepared by dissolving 2.05 g of sodium acetate, CH3COONa, in 85.0 mL of 0.10 Macetic Assume the volume change upon dissolving the sodium acetate is negligible. K₂ of CH3COOH is acid, CH3COOH(aq). 1.75 x 10-5. pH =arrow_forward(a) Using the expression Ka=[H+][A−]/[HA], explain how to determine which solution has the lower pH, 0.10MHF(aq) or 0.10MHC2H3O2(aq). Do not perform any numerical calculations. (b) Which solution has a higher percent ionization of the acid, a 0.10M solution of HC2H3O2(aq) or a 0.010M solution of HC2H3O2(aq) ? Justify your answer including the calculation of percent ionization for each solution.arrow_forward
- Calculate the change in pH when 3.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH₂ (aq) and 0.100 M in NH₂Cl(aq). Consult the table of ionization constants as needed. ΔΡΗ = Calculate the change in pH when 3.00 mL of 0.100 M NaOH is added to the original buffer solution. ApH =arrow_forwardB represents an acid-base indicator and behaves like a base. Its dissociation equilibrium in an aqueous solution can be written as: B(ac) + H2O(l) <-> +BH(ac) + OH(ac) If B (ac) is yellow +BH is red. Using Le Châtelier's principle, predict the color of the indicator by adding a few drops of the indicator to an aqueous solution of HCl and an aqueous solution of NaOH. Write the corresponding chemical reactions.arrow_forwardCalculate the equilibrium concentration of HC2O4−HC2O4− in a 0.20 mol L−1mol L−1 solution of oxalic acid. Express your answer to two significant figures and include the appropriate unitsarrow_forward
- Explain the chemistry behind the difference of pH between normal rainwater and acid rain. Please answer concisely.arrow_forward(a) Define a Lewis acid and a Lewis base. (b) Define an Arrhenius acid and an Arrhenius base. (c) Identify As2O5 as either a Brønsted-Lowry, a Lewis, or an Arrenius acid or base, and justify your answer to part (c) by writing a balanced chemical equation in showing As2O5 added to water.arrow_forward7 (a) Describe what happens when each of the following molecules is separately dissolved in water and illustrate with an equation in each case: (i) ethavois acid (CH;COOH) (ii) ammonia (NH3) (b) Identify the conjugate acids and bases in the substances mentioned in question 7(a) above.arrow_forward
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