The value of Ka for nitrous acid (HNO2) at 25 ∘Cis 4.5×10−4. You may want to reference(Pages 833 - 836) Section19.7 while completing this problem. |
Part A Write the chemical equation for the equilibrium that corresponds to Ka. Write the chemical equation for the equilibrium that corresponds to .
Part B Using the value of Ka, calculate ΔG∘ for the dissociation of nitrous acid in aqueous solution. Express your answer using three significant figures.
Part C What is the value of ΔG at equilibrium? Express your answer using one significant figure.
Part D What is the value of ΔG when [H+] = 5.6×10−2M , [NO−2] = 6.3×10−4M and [HNO2] = 0.21 M ? Express your answer using three significant figure.
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The value of Ka for nitrous acid (HNO2) at 25 ∘Cis 4.5×10−4. You may want to...
The value of Ka for nitrous acid (HNO2) at 25 ∘C is 4.5×10−4. You may want to reference (Pages 833 - 836) Section19.7 while completing this problem. 1. What is the value of ΔG when [H+] = 5.9×10−2M , [NO−2] = 6.3×10−4M and [HNO2] = 0.19 M ? Express your answer using three significant figure.
The value of Ka for nitrous acid (HNO2) at 25 ∘C is 4.5×10−4. Part D What is the value of AG when [H+] = 5.8 x 10-2M, [NOą] =6.4 x 10-4 M and (HNO2] = 0.21 M ? Express your answer using three significant figure. IVO AED A o 2 ? AG = Submit Previous Answers Request Answer X Incorrect; Try Again; 3 attempts remaining Recall that AG = AGº + RTinQ, where R is the gas constant, T is...
The KbKb for methylamine (CH3NH2)(CH3NH2) at 25 ∘C∘C is 4.4×10−44.4×10−4. Part B. By using the value of KbKb, calculate ΔG∘ΔG∘ for the equilibrium in part A. Part D. What is the value of ΔGΔG when [H+][H+] = 6.6×10−9 MM, [CH3NH+3][CH3NH3+] = 2.5×10−3 MM, and [CH3NH2][CH3NH2] = 9.70×10−2 MM? The value of KaKa for nitrous acid (HNO2)(HNO2) at 25 ∘C∘C is 4.5×10−44.5×10−4. You may want to reference (Pages 833 - 836) Section19.7 while completing this problem. 1. Using the value of...
Calculate the pH of a 0.383 M aqueous solution of nitrous acid (HNO2, Ka = 4.5×10-4) and the equilibrium concentrations of the weak acid and its conjugate base. pH = [HNO2 ]equilibrium = M [NO2- ]equilibrium = M
Nitrous acid, HNO2(aq), has a Ka of 4.5 x 10-4 at 25 °C. What is the pH of a solution that contains 1.0 M KNO2(aq) and 0.50 M HNO2(aq).
Nitrous acid, HNO2, has a Ka of 7.1 × 10−4. What are [H3O+], [NO2−], and [OH−] in 0.54 M HNO2?
LouiJL LUNCHILL Which of the following represents the Ka of nitrous acid, HNO2? [H+][N][0]2 [HNO2) None of these are correct. [+][Noz (HNO2] [**]*[noz] (HNO2] [H+][NO2.]. Submit Answer Tries 0/98 This discussion is closed.
Ka for nitrous acid, HNO2, is 4.50×10-4. Ka for hydrofluoric acid, HF, is 7.20×10-4. Ka for hydrocyanic acid, HCN, is 4.00×10-10. What is the formula for the strongest conjugate base? ______?____
a solution of nitrous acid (HNO2 , Ka=4.5*10^-4) has a pH OF 1.85. How many grams of nitrous acid are there in 100 ml of the solution?
Given the following acid dissociation constants, Ka (HNO2) = 4.0 x 10-4 Ka (HCN) = 4.0 x10-10 determine the equilibrium constant for the reaction below. HCN(aq) + NO2 - (aq) CN- (aq) + HNO2(aq)