Use the picture below to answer the following question: Simple Conductivity Tester mostly ions H* cF Battery mostly HC2H5O2 molecules C. Ophardt, o. 2003 Which light bulb in the picture above is connected to a solution with a strong acid? In your answer include what you know about dissociation and strength of an acid and provide details from the picture to support your response.

Use the picture below to answer the following question: Simple Conductivity Tester mostly ions H* cF Battery mostly HC2H5O2 molecules C. Ophardt, o. 2003 Which light bulb in the picture above is connected to a solution with a strong acid? In your answer include what you know about dissociation and strength of an acid and provide details from the picture to support your response.

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) What is the value of the equilibrium constant for the reaction of a strong acid with a weak base which has a Kb of 3.8E-5? H3O+(aq) + B(aq) ⇆ BH+(aq) + NO3-(aq) b) An aqueous solution is made of the diprotic acid H2A to a concentration of 0.15 M H2A. Ka1 = 3.0 x 10-4 and Ka2 = 2.5 x 10-9 What is the [A2-] in this solution? Your answer should have 2 significant figures and be expressed in scientific notation (i.e. 3.0 x 10-2 as 3.0e-2)
Why is the answer a & d?
Calculate the pH of a solution containing a salt AcNa derived from a strong base (NaOH) and a weak acid (AcH), like CH3COONa, KF, NaNO2 and so on. In this case two processes have to be considered: 1. Dissociation of the salt, within the assumption that the salt is a strong electrolyte: AcNa → Ac- + Na+, for instance: CH3COONa → CH3COO- + Na+ 2. the hydrolysis of the water Ac- + H2O ⇌ AcH + OH-, for example: CH3COO- + H2O ⇌ CH3COOH + OH- knowing that the initial concentration of the salt is 1.75 M and the acid dissociation constant, Ka , is 2.07e-7. What is the PH?
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a strong base Pe(OH)2 solution with (2.25x10^-4) M. Assume that the autoprotolysis of water does not contribute significantly to the OH- or H+ concentrations. Determine the pH of Pe(OH)2.
Dd.14.