Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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The pH for 0.050 M CH3NH2 (Kb for CH3NH2 = 4.0 X 10^-4 )?
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- Consider an aqueous solution that is 0.050 M in H2Se (Ka = 1.29 x 10-4) and 0.075 M in NaHSe. Out of the answer choices below, which is the only pH that could possibly be correct? (NOTE: The correct answer may or may not be the actual pH of the solution.) Group of answer choices 1.29 2.56 3.88 4.30arrow_forwardWhat is the pH of 0.28 M CH3NH3Br (Kb of CH3NH2 is 4.4x10^-4)arrow_forwardDetermine the pH of the molecules given in a 1L beaker containing 0.035M solution of the given molecule: NaNO2, C6H5CHCOOH, Ba(OH)2. (C6H5CHCOOH, Ka=6.3 x 10^-5, HNO2 Ka= 4.5 x 10^-4, CH3NH2, Kb= 5.0 x 10^-4).arrow_forward
- 3:21 2- 3C₂²- + 1 2 3 4 CI Complete the balanced chemical reaction for the following weak base with a strong acid. In this case, write the resulting acid and base as its own species in the reaction. NH3(aq) + HCl(aq) (s) Question 1 of 10 O Reset LO 5 6 OH- 7 8 ଇ H H₂O H3O+ ↑ x H₂O Tap here or pull up for additional resources Submit 9 11 (aq) O Narrow_forwardEach of the four flasks below contains the same volume of .10 M aqueous acid. All four acids are monoprotic, meaning that each acid molecule gives up one H+. The pH of each solution is as indicated. Flask A: pH=1.1 Flask B: pH=2.4 Flask C pH= 2.9 Flask D: pH=5.1 How much strong base is required to neutralize the initial amount of acid? A. All four solutions will require the same amount of base because they all contain acid of the same concentration B. The solution of pH=1.1 will require the most base since it is the strongest acid and has the highest concentration of H+ C. Neither (A) nor (B) is correct.arrow_forwardAmmonia, a weak base with a Kb value of 1.8 x 10^-5 (a) What is the pH of a 0.155 mol L^-1 ammonia solution? (b) What is the percent ionization of ammonia at this concentration?arrow_forward
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