For the diprotic weak acid H₁A, Kal = 3.2 × 10-6 and Ka2 = 6.3 × 10-9.What is the pH of a 0.0800 M solution of H,A? What are the equilibrium concentrations of H2A and A2 in this solution?Step 1: Make an equilibrium table for the molar concentrations at equilibrium after the first dissociation step.Concentration (M)H,A(aq)H+(aq) +HA (aq)initial0.080000change-I+x+xequilibriumExpress Kal in terms of the initial concentration of H,A and x, and then show the simplified expression when x is assumed tobe negligible compared to to the initial concentration.complete:Kal==3.89IncorrectDetermine the numerical value of x.x =6.3 ×10 9Msimplified: Kal≈ 3.9Incorrect

For H2AKa1 = Ka2 = Concentration of H2A = 0.0800 MWe have to determine the pH of the solution and…

For the diprotic weak acid H,A, Kal = 3.2 x 10 and Ka2 = 6.3 x 10-9 What is the pH of a 0.0800 M solution of H,A? What are the equilibrium concentrations of H2A and A2 in this solutio Step 1: Make an equilibrium table for the molar concentrations at equilibrium after the first dissociation step. Concentration (M) H,A(aq) 1 H+(aq) + HA (aq) initial 0.0800 0 0 change -X +x +x equilibrium Express Kal in terms of the initial concentration of H2A and x, and then show the simplified expression when x is assumed be negligible compared to to the initial concentration. complete: Kal= 3.89 Incorrect Determine the numerical value of x. simplified: Kal≈ 3.9 Incorrect

For the diprotic weak acid H,A, Kal = 3.2 x 10 and Ka2 = 6.3 x 10-9 What is the pH of a 0.0800 M solution of H,A? What are the equilibrium concentrations of H2A and A2 in this solutio Step 1: Make an equilibrium table for the molar concentrations at equilibrium after the first dissociation step. Concentration (M) H,A(aq) 1 H+(aq) + HA (aq) initial 0.0800 0 0 change -X +x +x equilibrium Express Kal in terms of the initial concentration of H2A and x, and then show the simplified expression when x is assumed be negligible compared to to the initial concentration. complete: Kal= 3.89 Incorrect Determine the numerical value of x. simplified: Kal≈ 3.9 Incorrect

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...

See similar textbooks

Similar questions

3.
HA is a weak acid. Select the correct dropdown value to correctly complete the incomplete concentration table below being used to determine the equilibrium concentrations of HA, H3O*, and A¯ of a 0.1300 M HA solution that has a pH of 3.60 at 25°C. HA(aq) + H,0(1) = H,0^(aq) + A-(aq) Initial 0.1300 Change Equilibrium (b) (a] The value for a is [ Select ] The value for b is [ Select ] What is the Ka of this weak acid? [ Select]
If the Ka of a reaction is equal to 1.8x10-5, which is favored- the products or the reactants? How would the pH change if a concentration of conjugate pairs increased from 0.01 M to 0.1 M?
5) Find the concentration of H30*(aq) in a 1.75 M solution of lactic acid, HC3H5O3, at 25°C. Ka= 1.38 x 10*. 6) Write the equilibrium expression for the ionization of HOI, and calculate the concentration of HOI(aq) in solution if [H3O*]=2.3 x 10° M and pKa = 10.7 at 25°C.
O ACIDS AND BASES Calculating the pH of a salt solution 1/5 Calculate the pH at 25 °C of a 0.63 M solution of sodium benzoate (NaC,H,CO,). Note that benzoic acid (HC,H;CO,) is a weak acid with a p K, of 4.20. Round your answer to 1 decimal place. PH = II
Nitrous acid, HNO2 has a Ka = 7.13 x 10-4. Construct an ICE table describing the ionization of 0.700 M HNO2. From the ICE table, estimate the following values: Find the pH Find the concentration of [NO2--] Find the extent of ionization, ?α
Complete the balanced molecular reaction for the following weak base with a strong acid: Na CIO2(aq) + H2SO«(aq) – 4- |2+ 3+ 04+ 1 4 6. 7 8 9 Do (s) (1) (g) (aq) Na CI S H H2O OH Reset x H2O Delete 1L LO
A patient presents itself to the emergency department in a critical condition. The patient’s blood was tested and the concentration of carbonic acid (H2CO3) was found to be 6.8 ×10-8 M and bicarbonate ion (HCO3-) 2.325 ×10-7 M Ka = 4.3 × 10-7 H2CO3(aq) ⇌ HCO3-(aq) + H+(aq) Show all calculations including equation(s) used. Calculate the pH of the patients’ blood. Based on your answer would you say the patient is suffering from Acidosis or Alkalosis?
← Sign in to your account → canvas < + X app.101edu.co school mail all apps Aktiv Chemistry beSocratic bartleby X G If the reaction quotient (Q) is larg X docs P Pearson+ Aktiv m HBOMax Answered: The following acid-bas x + Question 19 of 57 For the reaction of carbon monoxide and hydrogen, the equilibrium concentrations are 3.26 M CO and 1.06 M H₂. The equilibrium constant, Kc, is 0.118. Calculate the equilibrium concentration of CH₂OH(g). CO (g) + 2 H₂ (g) = CH3OH (g) 1 4 7 +/- 2 5 8 0.591 M 3 6 CO 9 0 T U Submit X R : C x 100
Calculate the equilibrium Molarity of HPO4^2-
4.