Chemical Principles in the Laboratory
11th Edition
ISBN: 9781305264434
Author: Emil Slowinski, Wayne C. Wolsey, Robert Rossi
Publisher: Brooks Cole
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Chapter 25, Problem 3ASA
The pH of a 0.10 MHOBr solution is 4.8.
- What is [H+] in that solution? ____________M
- What is [OBr-]? What is [HOBr]? (Where do the H+ and OBr- ions comes from?) ____________M; ____________M
- What is the value of Ka for HOBr? What is the value of pKa?____________ ____________
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If HNO3 is added to water, how does [OH-] change? How does pH change? (b) Use the pH values in Figure 16.5 to estimate the pH of a solution with [OH-] = 0.014 M. Is the solution acidic or basic? (c) If pH = 6.6, first estimate and then calculate the molar concentrations of OH-(aq) and H+(aq) in the solution. Figure 16.5
a) Enough of a monoprotic acid is dissolved in water to produce a 1.291.29 M solution. The pH of the resulting solution is 2.832.83. Calculate the Ka for the acid.
b)
i) Determine the [OH−] , pH, and pOH of a solution with a [H+] of 8.6×10−10 M at 25 °C.
ii) Determine the [H+] , pH, and pOH of a solution with an [OH−] of 0.028 M at 25 °C.
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the ph of a 0.010M solution of just HOCL in water is 4.8 . What is H+ in that solution? b) what is [OCL-]? What is [HOCL] ? Where do the H+ and OCL- ions come from ? what is the value of K4 for HOCL? WHat is the value of pk4 for HOCl?
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Chemical Principles in the Laboratory
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General Chemistry | Acids & Bases; Author: Ninja Nerd;https://www.youtube.com/watch?v=AOr_5tbgfQ0;License: Standard YouTube License, CC-BY