Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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At 50°C the Kw of pure water is 5.476 x 10-14. Calculate the H3O+ and OH- concentrations, and then find
the pH and pOH.
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- A solution is prepared at 25 °C that is initially 0.48 M in diethylamine ((C,H5)¸NH), a weak base with K,=1.3 × 10 -3 and 0.024M in diethylammonium bromide ((C,H5) NH,Br). Calculate the pH of the solution. Round your answer to 2 decimal places. pH olo Ararrow_forwardWhat is the pH of a solution that is 0.21 M CH3NH2 (methylamine) and 0.31 M CH3NH3Cl (methylammonium chloride)? (Assume Kw is 1.0 ✕ 10−14.)arrow_forwardWhat is the concentration of hydroxide ion in a 0.76 M aqueous solution of hydroxylamine, NH2OH? (Assume the value of Kw is 1.0 10-14.) what is M ? What is the pH ?arrow_forward
- Calculate the pH of the mixture of 105 mL of 0.195 mol/L hydrazine (H2NNH2) with 95 mL of a 0.215 mol/L H2NNH3Br solutionGive an answer to at least 3 decimal places. Next, calculate the pH of this same solution if 12.00 mL of 0.300 mol/L HNO3 is added.Give an answer with at least 3 decimal places.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_forwardCalculate the pH of a solution that is 0.374 M CH3COOH and 0.489 M CH3COONa. Ka of CH3COOH is 1.8 * 10^-5.arrow_forward
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