MISSED THIS? Watch KCV 16.3; Read Section 16.3. You can click on the Review link to access the section in your e Text. Both HCO₁ and HS are amphoteric Part A Enter an equation to show how HCO, can act as a base with HS acting as an acid. Express your answer as a chemical equation. Identify all of the phases in your answer. ΑΣΦΑ ? HCO +HSH,CO, +S²- A chemical reaction does not occur for this question. Check your placement of subscripts and superscripts. You can also review how to insert subscripts and more No credit lost. Try again. Submit Part B Previous Answers Request Answer CI Enter an equation to show how HCO, can act as an acid with HS acting as a base. Express your answer as a chemical equation. Identify all of the phases in your answer. AX A chemical reaction does not occur for this question Submit Besest Answer

MISSED THIS? Watch KCV 16.3; Read Section 16.3. You can click on the Review link to access the section in your e Text. Both HCO₁ and HS are amphoteric Part A Enter an equation to show how HCO, can act as a base with HS acting as an acid. Express your answer as a chemical equation. Identify all of the phases in your answer. ΑΣΦΑ ? HCO +HSH,CO, +S²- A chemical reaction does not occur for this question. Check your placement of subscripts and superscripts. You can also review how to insert subscripts and more No credit lost. Try again. Submit Part B Previous Answers Request Answer CI Enter an equation to show how HCO, can act as an acid with HS acting as a base. Express your answer as a chemical equation. Identify all of the phases in your answer. AX A chemical reaction does not occur for this question Submit Besest Answer

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 119QRT

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Oxalic acid (H2C2O4) is a diprotic acid with Ka1=5.6×10-1 and Ka2=1.5×10-4. Oxalate ion (C2O42-) also has two base dissociation constants, Kb(1) =6.5×10-11 and Kb2=1.8×10-14. Based on these values, deduce the formula to compute the base dissociation constants of oxalate ion in terms of Kw and Ka1 or Ka2.
Oxalic acid (H2C2O4) is a diprotic acid with Ka1 = 5.6x10-1 and Ka2 = 1.5x10-4. Oxalate ion (C2O42-) also has two base dissociation constants, Kb1 = 6.5x10-11 and Kb2 = 1.8x10-14. Based on thesevalues, deduce the formula to compute the base dissociationconstants of oxalate ion in terms of Kw and Ka1 or Ka2
Both H2PO3−H2PO3− and HS−HS− are amphoteric. Write an equation to show how H2PO3−H2PO3− can act as a base with HS−HS− acting as an acid. Express your answer as a chemical equation. Identify all of the phases in your answer. then Write an equation to show how H2PO3−H2PO3− can act as an acid with HS−HS− acting as a base. Express your answer as a chemical equation. Identify all of the phases in your answer.
Your consulting firm wants you to oversee the swimming pool disinfection arm of their business. Your new boss thinks that switching disinfectants from Cl2 gas to bleach (NaOCl) will save cost by eliminating engineering safety controls for Cl2 gas storage. The total acid or conjugate base is added to swimming pools at a concentration of 5*10^-3 M. Assuming activity coefficient = 1, algebraically calculate the pH of the pool where 5*10^-3 M of NaOCl is added. For any simplifications you make, include checks of your assumptions to validate your calculations.
5,Calculate the [OH-]of the solution with pH=10.50 Group of answer choices 1.05 x 10-10 5.0 x 10-10 3.2 x 10-10 3.2 x 10-4 6, Use the Ka values for the following acids to find the strongest conjugate base: HSO4- 1.2 x 10-2H2PO4- 6.3 x 10-8HCO3- 4.7 x 10-11 Group of answer choices A, H3PO4 B, H2SO4 C, HPO42- D, H2CO3 E, CO32- F, SO42-
What is the pH of a solution prepared by combining 0.696 mol of a weak acid (Ka = 5.5 x 10-5) with 0.516 mol of the salt containing its conjugate base in 3.4 L of water? Report your answer to the hundredths place and do not include units.
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The acid ionization constants for species that are listed below can be found by using data given in the following tables: Acid Ka1 Ka2 Ka3 H3PO4 7.5 x 10–3 6.2 x 10–8 4.2 x 10–13 H2CO3 4.3 x 10–7 5.6 x 10–11 HNO2 4.5 x 10–4 HIO3 1.7 x 10–1 Base Kb NH3 1.8 x 10–5 Which of the following is the weakest acid? HCO3– HNO2 NH4+ HIO3 H2PO4–
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Reacting GeO2 with H2O forms the tetraprotic (four H+ ions) acid, H4GeO4. On a piece of paper, write down the chemical equations for the four acid dissociation equilibria. Match each chemical species below with its correct role in this polyprotic acid system. H4GeO4 H3GeO4 - H2GeO4 2- HGeO4 3- GeO4 4- [ Choose ] the conjugate base of H3GeO4 - the acid in the second H+ dissociation this species' conjugate acid is HGeO4 3- the conjugate base in the third H+ dissociation the conjugate acid of H3GeO4 -
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