17. Determine the pH of the resulting solutions when the following reagents aremixed.d. 25.00mL of 0.1000M HCIO, mixed with 25.00mL of 0.1000M KOHe. 15.00mL of 0.1000M CH;NH2 mixed with 25.00mL of 0.1500M HCI

PH is calculated by using the concentration of H+,PH= -log [H+]PH range is in between 0 to 14 7 PH…

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Determine the pH of the resulting solutions

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.31QE

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Concept explainers

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Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

17. Determine the pH of the resulting solutions when the following reagents are
mixed.
d. 25.00mL of 0.1000M HCIO, mixed with 25.00mL of 0.1000M KOH
e. 15.00mL of 0.1000M CH;NH2 mixed with 25.00mL of 0.1500M HCI

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How many grams of HI should be added to 265 mL of 0.215 M HCI so that the resulting solution has a pH of 0.38? Assume that the addition of HI does not change the volume of the resulting solution.
. Which component of a buffered solution is capable of combining with an added strong acid? Using your example from Exercise 60, show how this component would react with added HC1.
A solution is made by diluting 25.0 mL of concentrated HCl (37% by weight; density = 1.19 g/mL) to exactly 500 mL. Calculate the pH of the resulting solution.
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