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Ch.16 - Acid-Base Equilibria
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All textbooksBrown 14th EditionCh.16 - Acid-Base EquilibriaProblem 4c

Chapter 16, Problem 4c

The probe of the pH meter shown here is sitting in a beaker that contains a clear liquid. (c) Why is the temperature given on the pH meter?

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Hey everyone, we're told that the ph of a clear liquid was determined using a ph meter, as shown below. Is the temperature given, with the ph reading necessary First, let's think about what we know about a ph scale. We know that it's based on the kw of water and r k w is our equilibrium constant, which is temperature dependent. So as we've learned, we have different values of KW at different temperatures. So when it's not at 25°C, our KW is not equal to our 1.0 times 10 to the -14. So to answer this question, our answer would be yes. The given temperature. Is it necessary since our k w and our ph our temperature dependent, and this is going to be our final answer. Now, I hope that made sense. And let us know if you have any questions.
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At 50 °C, the ion-product constant for H2O has the value Kw = 5.48 * 10-14. (a) What is the pH of pure water at 50 °C? (b) Based on the change in Kw with temperature, predict whether ΔH is positive, negative, or zero for the autoionization reaction of water: 2 H2O1l2 Δ H3O+1aq2 + OH-1aq2

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The indicator methyl orange has been added to both of the following solutions. Based on the colors, classify each statement as true or false: (a) The pH of solution A is definitely less than 7.00.

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Textbook Question

The probe of the pH meter shown here is sitting in a beaker that contains a clear liquid. You are told the liquid is pure water, a solution of HCl(aq), or a solution of KOH(aq). (b) If the liquid is one of the solutions, what is its molarity?

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The following diagrams represent aqueous solutions of three acids, HX, HY, and HZ. The water molecules have been omitted for clarity, and the hydrated proton is represented as H+ rather than H3O+. (a) Which of the acids is a strong acid? Explain.

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The following diagrams represent aqueous solutions of three acids, HX, HY, and HZ. The water molecules have been omitted for clarity, and the hydrated proton is represented as H+ rather than H3O+.(b) Which acid would have the smallest aciddissociation constant, Ka?

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The following diagrams represent aqueous solutions of three acids, HX, HY, and HZ. The water molecules have been omitted for clarity, and the hydrated proton is represented as H+ rather than H3O+.(c) Which solution would have the highest pH?

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