QUESTION 6A titration of 45.0 mL of 0.17M HNO2 with a 0.25M LIOH solution. What is the pH of the solution after 27.0 mL of LIOH are addWrite answer in decimal form to two decimal places.K =1.0x1014pH = pka + log[A]/[HA]pH = -log[H,O)14 pH+ pOH%3DQUESTION 7What is the molar solubility of YF in water? Ken = 8.62x10Write answer in scientific nototion to the two significant figures. When writing scientific notation use "E". For exomple, 0.0003 would be4.2E-6O Type here to searchPCP

Given molarity of HNO3 = 0.17 M Volume = 45 mL = 0.045 L So, Number of moles of strong acid HNO3 =…

QUESTION 6 A titration of 45.0 mL of 0.17M HNO2 with a 0.25M LIOH solution. What is the pH of the solution after 27.0 mL of LIOH are add Write answer in decimal form to two decimal places. K = 1.0x1014 pH = pKa + log[A]/[HA] pH = -log[H,0] 14 = pH + pOH

QUESTION 6 A titration of 45.0 mL of 0.17M HNO2 with a 0.25M LIOH solution. What is the pH of the solution after 27.0 mL of LIOH are add Write answer in decimal form to two decimal places. K = 1.0x1014 pH = pKa + log[A]/[HA] pH = -log[H,0] 14 = pH + pOH

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

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