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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Transcribed Image Text:11. Calculate the pH of a .075 M orange juice solution (Ka citric acid = 1.5 x 103).
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- A certain base has a Kb of 7.8 × 10-6 . What concentration of the base will produce a pH of 11.32?arrow_forwardWhat is the pH of a 0.862 M NH3 solution that has a Kb = 1.8 x 10-5?arrow_forwardWhat is the pH of a 0.1055 M CH3COOH solution (K, = 1.75 x 10-5)? A) 2.770 B) 2.867 3.188 D 8.474arrow_forward
- 3 Calculate the OH concentration and pH of a 1.8 x 10 M aqueous solution of sodium cyanide, N.CN. Finally, calculate the CN concentration. ( K.(HCN) = 4.9 x 10 10) [OH ]= M pH = [CN ] =[ Marrow_forwardFind the pH of a 0.600 M solution of methylamine CH3NH2. Kb = 4.4 x 10-4. %3Darrow_forwardEach solution below has pH = 4.5. Which solution most effectively maintains pH between 4.0 and 5.0 upon addition of a small amount of strong acid or base? O 1.00 M NaF +0.050 M HF. K₂(HF) = 6.3 x 10-4 O 2.1 M NaH₂PO4 + 0.0085 M H3PO4. Ka1(H3PO4) = 7.5 × 10-³ 0.80 M NaNO₂ + 0.055 M HNO₂. Ka(HNO2, nitrous acid) = 4.6 x 10-4 O 1.0 M NaC7H502 +0.50 M HC7H5O2. Ka(HC₂H5O₂, benzoic acid) = 6.3 × 10-5arrow_forward
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