Scientists use the pH scale to represent the level of acidity or alkalinity of a liquid. This is based on the molar concentration of hydrogen ions, [H+]. Since thevalues of [H+] vary over a large range, 1 x 10° mole per liter to 1 x 10-14 mole per liter (mol/L), a logarithmic scale is used to compute pH. The formulapH= -log[H+]represents the pH of a liquid as a function of its concentration of hydrogen ions, [H+].The pH scale ranges from 0 to 14. Pure water is taken as neutral having a pH of 7. A pH less than 7 is acidic. A pH greater than 7 is alkaline (or basic).For this exercise, use the formula for pH. Round pH values to 1 decimal place.Lemon juice Wine10⁰0 1 2 3 4 5 6 7 8 9 10 11 12 13 1410-2Acidic10-10-7AmmoniaWater(neutral)Bleach10-10 10-12AlkalinepH10-14 [H+1 11Ammonia and oven cleaner are both bases. Their [H+] values are 1.3 × 10¹¹ mol/L and 6.3 × 10-¹4(a) Find the pH for ammonia.(b) Find the pH for oven cleaner.(c) Which substance is more basic?Part: 0 / 3Part 1 of 3(a) Find the pH for ammonia.The pH for ammonia is approximatelyX3mol/L, respectively.

pH is defined as negative logarithm of hydrogen ion concentration pH=-log[H+] Substance that has pH…

Ammonia and oven cleaner are both bases. Their [H+] values are 1.3 x 10 11 (a) Find the pH for ammonia. (b) Find the pH for oven cleaner. (c) Which substance is more basic? Part: 0/3 Part 1 of 3 (a) Find the pH for ammonia. The pH for ammonia is approximately X 5 mol/L and 6.3 × 10 -14 mol/L, respectively.

Ammonia and oven cleaner are both bases. Their [H+] values are 1.3 x 10 11 (a) Find the pH for ammonia. (b) Find the pH for oven cleaner. (c) Which substance is more basic? Part: 0/3 Part 1 of 3 (a) Find the pH for ammonia. The pH for ammonia is approximately X 5 mol/L and 6.3 × 10 -14 mol/L, respectively.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 60QAP: Consider a 0.33 M solution of the diprotic acid H2X. H2X H+(aq)+ HX(aq)Ka1=3.3 10 4 HX H+(aq)+...

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