Pre-Lab Quiz 6 - 2 E 587 mL HNO 2 413 mL KNO Question 3 For...

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http://chemmac1.usc.edu/cttccgi/randquiz.cgi 1 of 2 Web Quiz You can login to this page multiple times but you cannot take the quiz more than once.. Submit your answer for grading by Clicking on the "Grade Answers" button at the bottom of the page only when you are sure of your answers. Question # 1 Calculate the [H + ] in a solution that is 0.10 M in NaF and 0.20 in HF. ( K a = 7.2 x 10 -4 ) A. 0.20 M B. 7.0 x 10 -4 M C. 1.4 x 10 -3 M D. 3.5 x 10 -4 M E. none of these Question # 2 You have solutions of 0.200 M HNO 2 and 0.200 M KNO 2 ( K a for HNO 2 = 4.00 x 10 -4 ). A buffer of pH 3.000 is needed. What volumes of HNO 2 and KNO 2 are required to make 1 liter of buffered solution? A. 500 mL of each B. 286 mL HNO 2 ; 714 mL KNO 2 C. 413 mL HNO 2 ; 587 mL KNO 2 D. 714 mL HNO
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Unformatted text preview: 2 E. 587 mL HNO 2 ; 413 mL KNO Question # 3 For a solution equimolar in HCN and NaCN, which statement is false? http://chemmac1.usc.edu/cttccgi/randquiz.cgi 2 of 2 A. This is an example of the common ion effect. B. The [H + ] is larger than it would be if only the HCN was in solution. C. The [H + ] is equal to the K a . D. Addition of more NaCN will shift the acid dissociation equilibrium of HCN to the left. E. Addition of NaOH will increase [CN-] and decrease [HCN]. Question # 4 For ammonia, K b is 1.8 x 10-5 . To make a buffered solution of pH 10.0, the ratio of NH 4 Cl to NH 3 must be: A. 1.8 : 1 B. 1 : 1.8 C. 0.18 : 1 D. 1 : 0.18 E. none of these Grade Answers...
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