At 25 °C phosphoric acid, H3PO4, has the following equilibrium constants:Part AKa7.5 x 10-36.2 x 10-8What is the pH of a solution of 0.25 mol L-1 KPO4, potassium phosphate?4.2 x 10-13Express your answer numerically to the hundredths place.• View Available Hint(s)pH =SubmitPart BWhat is the pH of a solution of 0.350 mol L- K2HP04, potassium hydrogen phosphate?Express your answer numerically to the hundredths place.• View Available Hint(s)pH =SubmitPart CWhat is the pH of a solution of 0.400 mol L-1 KH PO4, potassium dihydrogen phosphate?Express your answer numerically to the hundredths place.• View Available Hint(s)pH =

Answered: Image /qna-images/answer/8dbaa467-a8b5-4d1d-a56a-d7e53bdefe04.jpg

At 25 °C phosphoric acid, H3PO4, has the following equilibrium constants: Part A = 7.5 x 103 Ka K. - 6.2 x 10-8 What is the pH of a solution of 0.25 mol L- K3PO4. potassium phosphate? K. 4.2 x 10-13 Express your answer numerically to the hundredths place. • View Available Hint(s) pH = Submit Part B What is the pH of a solution of 0.350 mol L K2HPO4. potassium hydrogen phosphate? Express your answer numerically to the hundredths place. • View Available Hint(s) pH = Submit Part C What is the pH of a solution of 0.400 mol L-1 KH2PO4, potassium dihydrogen phosphate? Express your answer numerically to the hundredths place. • View Available Hint(s) pH =

At 25 °C phosphoric acid, H3PO4, has the following equilibrium constants: Part A = 7.5 x 103 Ka K. - 6.2 x 10-8 What is the pH of a solution of 0.25 mol L- K3PO4. potassium phosphate? K. 4.2 x 10-13 Express your answer numerically to the hundredths place. • View Available Hint(s) pH = Submit Part B What is the pH of a solution of 0.350 mol L K2HPO4. potassium hydrogen phosphate? Express your answer numerically to the hundredths place. • View Available Hint(s) pH = Submit Part C What is the pH of a solution of 0.400 mol L-1 KH2PO4, potassium dihydrogen phosphate? Express your answer numerically to the hundredths place. • View Available Hint(s) pH =

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.66PAE

See similar textbooks

Similar questions

Table 13-4 lists the stepwise Ka values for some polyprotic acids. What is the difference between a monoprotic acid, a diprotic acid, and a triprotic acid? Most polyprotic acids are weak acids; the major exception is H2SO4. To solve for the pH of a solution of H2SO4, you must generally solve a strong acid problem as well as a weak acid problem. Explain. Write out the reactions that refer to Ka1 and Ka2 for H2SO4. For H3PO4, Ka1 = 7.5 103, Ka2 = 6.2 108, and Ka3= 4.8 1013. Write out the reactions that refer to the Ka1, Ka2and Ka3equilibrium constants. What are the three acids in a solution of H3PO4? Which acid is strongest? What are the three conjugate bases in a solution of H3PO4? Which conjugate base is strongest? Summarize the strategy for calculating the pH of a polyprotic acid in water.
Amino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H) and the amine group (NHR) are protonated. However, as the pH of the solution increases (say, by adding base), the carboxylic acid proton is removed, usually at a pH between 2 and 3. In a middle range of pHs, therefore, the amine group is protonated, but the carboxylic acid group has lost the proton. (This is called a zwitterion.) At more basic pH values, the amine proton is dissociated. What is the pH of a 0.20 M solution of alanine hydrochloride, [NH3CHCH3CO2H]Cl?
Write the equilibrium-constant expressions and obtain numerical values for each constant in (c) the acidic dissociation of methyl ammonium hydrochloride, CH3NH3Cl. (d) the basic dissociation of NaNO2. (e) the dissociation of H3AsO3 to H3O+ and AsO33-
1) Vinegar sold commercially is typically 0.8−1.0 M acetic acid. A 1.00 M solution of acetic acid is measured by its pH to have an equilibrium concentration of 4.19×10−3 M for both acetate ions and hydronium ions at room temperature. Assuming [HOAc]0 = 1.00 M, what is the equilibrium concentration of undissociated acetic acid [HOAc]eq to the correct number of significant figures?
Palmitic Acid, CH3(CH2)14COOH, found in both bacon fat and many soaps. Palmitic acid partially ionizes in water. Write a balanced chemical reaction for the dissociation of palmitic acid into its conjugate base and hydrogen ion. Write an expression for the equilibrium constant for palmitic acid. The equilibrium concentrations are [CH3(CH2)14COOH] = 0.1 M and [H+] = [CH3COO-] = 0.0133352 M. Calculate the equilibrium constant of ionization KA. Calculate the pKA of palmitic acid. Draw (by hand) the titration curve for palmitic acid. Please label your axes appropriately.
Write the expression for the acid-dissociation constant Ka for HC4H7O2. (Concentration equilibrium expressions take the general form: Kc = [C]c / [A]a . [B]b. Subscripts and superscripts that include letters must be enclosed in braces {}.)
A solution of sodium acetate is prepared using 0.56 mol L-1 NaOH as the solvent. The pKapKa of acetic acid is 4.75 . The concentration of sodium acetate after mixing, before any reaction takes place is 0.44 mol L-1 . Calculate the equilibrium concentrations of all acid species: [ CH3COOH ], [ CH3COO- ], the pH and the pOH in the solution. Some assumptions may not work, on the other hand, if you do not make the correct assumptions first, the quadratic formula will give you the wrong answer. [ CH3COOH ] = ___mol L-1 , [ CH3COO- ] = ___mol L-1 , pH = ___ pOH = ____
Acetic acid is a weak acid, meaning it does not fully dissociate in water. Instead, there is an equilibrium between the dissolved but undissociated molecule and the component ions: HOAc (aq) + H2O (l) ⇌ H3O+ (aq) + OAc– (aq)OAc– is an abbreviation for the acetate ion, CH3COO–, and H3O+ is the hydronium ion (lone protons, H+ (aq), do not exist!). (a) Write the equilibrium constant expression for the dissociation of acetic acid. (b) Vinegar sold commercially is typically 0.8 − 1.0 M acetic acid. A 1.00 M solution of acetic acid is measured by its pH to have an equilibrium concentration of 4.19×10−3 M for both acetate ions and hydronium ions at room temperature. Assuming [HOAc]0 = 1.00M, what is the equilibrium concentration of undissociated acetic acid [HOAc]eq to the correct number of significant figures? (c) What is the value of the equilibrium constant Keq for the dissociation according to the concentrations from part (b)? (d) When starting with completely un-dissociated…
15) 0.28 grams of sodium hydroxide are added to 40.0 mL of 0.25 M formic acid. Calculate the pH of the resulting solution. K, for the formate ion = 5.88 x 10-1.: * A) 3.40 B) 4.14 C) 9.83 D) 10.57
Calculate the pH of a solution prepared by dissolving 1.75 g of sodium acetate, CH3COON,, in 53.5 mL of 0.15 M acetic acid, CH3COOH(aq). Assume the volume change upon dissolving the sodium acetate is negligible. Ka of CH3COOH is 1.75 x 10-5.
The equilibrium constant for an acid is called the acid ionization constant (Ka). If acetic acid (weak acid, HC2H3O2) is placed into water, it ionizes to H+ and C2H3O2- with a Ka of 1.82 x 10-5. Determine the pH of the solution when 20.0 g HC2H3O2 (s) is added to water, with a final volume of 1000. mL?
Calculate the pOH of a 0.560 mol/L solution of hydrosulfuric acid which has aka of 1.1 x 10-7 . Determine the percent ionization of this acid.