31/1 pointBalance the reaction below and select all correct statements:CH3OH(aq) + Cr2O72(aq) CH2O(aq) + Cr3+(aq); acidicThe coefficient of H+ is 8The coefficient for water is 7The coefficient for CH3OH is 1The coefficient for Cr 3+ is 2

Let's try to balance the reaction in acidic solution. Step 1: DIVIDE THE REACTION INTO HALF…

Answered: 3 1/1 point Balance the reaction below…

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 29QRT

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Consider a salt of a weak base and a weak acid such as ammonium cyanide. Both the NH4+ and CN ions interact with water in aqueous solution, but the net reaction can be considered as a proton transfer from NH4+ to CN. NH4+(aq) + CN(aq) NH3(aq) + HCN(aq) (a) Show that the equilibrium constant for this reaction, Kact, is 1. Knet=KaKbKw where Ka is the ionization constant for the weak acid NH4+ and Kb, is the constant for the weak base CN. (b) Calculate Knet values fur each of the following, NH4CN, NH4CH3CO2, and NH4K Which salt has the largest value of Kact, and why? (c) Predict whether a solution of each of the compounds in (b) is acidic or basic. Explain how you made this prediction (Yon do not need a calculation to make this prediction.)
What are the major species in solution after NaHSO4 is dissolved in water? What happens to the pH of the solution as more NaHSO4 is added? Why? Would the results vary if baking soda (NaHCO3) were used instead?
Consider a 0.33 M solution of the diprotic acid H2X. H2X H+(aq)+ HX(aq)Ka1=3.3 10 4 HX H+(aq)+ X2(aq)Ka2=9.7 10 8 Calculate the pH of the solution and estimate [HX-] and [X2-].
Consider these acids (a) Arrange the acids in order of increasing acid strength from weakest to strongest. (b) Which acid has the smallest pKa value?
Calculate the pKa value for each of the following acids. a. Nitrous acid (HNO2), Ka = 4.5 104 b. Carbonic acid (H2CO3), Ka = 4.3 107 c. Dihydrogen phosphate ion (H2PO4), Ka = 6.2 108 d. Sulfurous acid (H2SO3), Ka = 1.5 102
The pH of human blood is steady at a value of approximately 7.4 owing to the following equilibrium reactions: CO2(aq)+H2O(l)H2CO3(aq)H2CO3(aq)+H+(aq) Acids formed during normal cellular respiration react with the HCO3 to form carbonic acid, which is in equilibrium with CO2(aq) and H2O(l). During vigorous exercise, a persons H2CO3 blood levels were 26.3 mM whereas his CO2 levels were 1.63 mM. On resting, the H2CO3 levels declined to 24.9 mM. What was the CO2 blood level at rest?
What is the ionization constant at 25 C for the weak acid (CH3)2 NH2+, the conjugate acid of the weak base (CH3)2NH, Kb=5.9104?
G.107.
Classify the following reactions in solutions as acidic or basic.
r 3C₂²- 1 Write the acidic ionization equation for HCI. Be sure to include the proper phases for all species within the reaction. HCl(aq) + H₂O (1)→ H₂O* + Cl(aq) 2 3 (s) OH™ Tap here or put up for additional resources ( H₂O* Reset 4 Question 24 of 55 (1) LO 5 CI 6 7 (g) H₂O ↑ 8 H 9 (aq) X 0 x H₂O LIE 46%E Submit
30. In the reaction HCl(aq) + H₂O(l) ⇒Cl¯(aq)+ H3O+ (aq) does water act as a Brønsted-Lowry acid, a Brønsted-Lowry base, or neither, or both? (A) Neither as an acid nor as a base; water is neutral (B) Both an acid and a base. (C) An acid (D) A base (E) Depends temperature
Complete the balanced neutralization equation for the reaction below:

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3 1/1 point Balance the reaction below and select all correct statements: CH3OH(aq) + Cr2O72(aq) CH2O(aq) + Cr3+(aq); acidic The coefficient of H+ is 8 The coefficient for water is 7 The coefficient for CH3OH is 1 The coefficient for Cr 3+ is 2