Substance to be tested Tap water Vinegar/acetic acid Milk of magnesia (Mg(OH)2) Coffee (make liquid solution) Green tea (make liquid solution) Liquid soap pH 0 Estimated pH based on color from Is this substance an acid, a base, or universal indicator paper pH-neutral? pH Scale for Part A: Add the tested substances to the pH scale below. Orange juice is provided as an example. Orange juice pH 3.9 solut 2 pH 7 pH 14

Substance to be tested Tap water Vinegar/acetic acid Milk of magnesia (Mg(OH)2) Coffee (make liquid solution) Green tea (make liquid solution) Liquid soap pH 0 Estimated pH based on color from Is this substance an acid, a base, or universal indicator paper pH-neutral? pH Scale for Part A: Add the tested substances to the pH scale below. Orange juice is provided as an example. Orange juice pH 3.9 solut 2 pH 7 pH 14

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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A new drug obtained from a plant was found to be a weak organic base. A solution of this weak base has a concentration of 0.0100 M, and a pH of 10.80 blank 1: write the pOH blank 2: write the [OH-] to 3 significant digits *DO NOT use scientific notation, spaces, or units blank 3: write the Kb value to 3 significant digits *DO NOT use scientific notation, spaces, or units
What volume of a concentrated HCl solution, which is 36.0% HCl by mass and has a density of 1.179 g/mL, should be used to make 5.10 L of an HCl solution with a pH of 1.60? Express your answer to two significant figures and include the appropriate units. HẢ ? V = Value Units
Negative ions, designated by the notation [OH-] are always present in any acid or base. The concentration, [OH-], of these ions is related to [H*] by the equation [OH-] [H] = 10-14 moles per liter. Find the concentrations of [OH¯] and [H*] in moles per liter for the substances with the given pH value. pH = 12 ... The concentration of [H*] is moles per liter. (Type your answer using exponential notation.) The concentration of [OH-] is moles per liter. (Type your answer using exponential notation.)
How do I calculate the theoretical pH for these? Mass of Sample, g Volume H20, mL Concentration Solution (M) Experimental pH Theoretical pH NaH2PO4 0.609 30.0 0.169 4.42 Na2HPO4 ●7H2O 0.608 30.0 0.076 8.45 Na3PO4 ●12H2O 0.224 10.0 0.0196 11.96
Part A If the pH of Solution 1 is 11.90, what is [H3O+]? Express your answer to two significant figures. Part B If the pH of Solution 1 is 11.90, what is [OH−]? Express your answer to two significant figures. Part D Solution 2 is a neutral solution. What is [H3O+] of Solution 2? Express your answer to two significant figures. Part E If the solution is neutral, what is [OH−]? Express your answer to two significant figures. Part G For Solution 3, if [H3O+] in the solution is 1.7×10−12M, what is [OH−] for this solution? Express your answer to two significant figures. Part H f [H3O+] in Solution 3 is 1.7×10−12M, what is the pH for this solution? Express your answer using two decimal places. Part I If [H3O+] in Solution 3 is 1.7×10−12M, is Solution 3 acidic, basic, or neutral
This is a multi-answer question. Please type your properly rounded answers in the next three questions (starting with this one): Calculate the pH of a 0.70 M solution of sodium sulfite, Na2SO3. Also calculate the concentrations of HSO3 and H₂SO3. Type the properly rounded pH below:
was is the correct sig figs
A stock solution of hydrochloric acid has a concentration of 0.1200M. It is diluted by transferring 10.00 mL to a 100mL volumetric flask using a volumetric pipette. Based on calculations it is found the pH is 1.92. Using the solution that was diluted, prepare a solution with a pH of 2.912. What volume of the diluted solution should you dilute to 100.00 mL to make this solution?
10) A solution is created by dissolving 14.2 grams of HCl (a strong acid) into water, making 2.63 Liters ofsolution. Calculate the Molarity of HCl, the [H+], and the pH of the solution. 10. M HCl = 0.148 M / [H+] = 0.148 M / pH = 0.829 Show step by step solutions 11) A basic solution is prepared to a measured pH of 12.45. Calculate the [OH-] and the [H+] of this solution [H+] = 3.548 x 10-13 M / [OH -] = 2.818 x 10-2 M Show step by step solutions
A typical vitamin C tablet (containing pure ascorbic acid, H₂C6H606) weighs 500 mg. One vitamin C tablet is dissolved in enough water to make 240.0 mL of solution. Calculate the pH of this solution. Ascorbic acid is a diprotic acid. For H₂C6H606, Ka1 = 7.9×10-5 and Ka2 = 1.6x10-12. pH = Submit Answer [References] Try Another Version 1 item attempt remaining