What is the pH of a 1.00 M solution of sodium sulfate
(NaHSO4)?
You can use the equilibrium constants from number 1 to figure out
the answer. (Ka1 = large
Ka2 = 1.2 x 10-2 )
What is the pH of a 1.00 M solution of sodium sulfate (NaHSO4)? You can use...
What is the pH of a 1.00 M solution of disodium sulfate (Na2SO4)? You can calculate the Kb from the Ka values given in the question 1. (Ka1 = large Ka2 = 1.2 x 10-2) 7.94 8.02 6.01 7.96
Calculate the pH of 1.00 x 10^-2 M oxalic acid solution. Calculate the pH of 1 x 10^-2 M solution of sodium oxalate. Ka1 = 5.62 x 10^-2, Ka2 = 5.42 x 10^-5
Calculate the pH when 200.0 mL of a 1.00 M solution of H2A (Ka1 = 1.0 x 10–6, Ka2 = 1.0 x 10–10) is titrated with the following volumes of 1.00 M NaOH. 250.0 mL of 1.00 M NaOH Group of answer choices
What is the PH of a 100 mM solution of sulfuric acid (H2SO4)? Ka1=Large Ka2=1.2x10^-2 A. 2.02 B. -0.96 C. 1.00 D. 1.9 E. 0.96
What is the pH of a solution made by mixing 100. mL of 0.010 M KHP (potassium hydrogen phthalate) and 100. mL of 0.032 M Na2P (sodium phthalate). Phthalic acid (H2P) has the following ionization constants: Ka1 = 1.122 x 10-3 Ka2 = 3.908 x 10-6
What is the pH of a 1 L solution containing 2 mol of sodium hydrogen sulfate (NaHSO4)? Ka for hydrogen sulfate = 1 x 10-2. Select one: O a. 0.8 O b. 1.0 6.0 d. 3.0 e. 2.0 ☺
A 0.200 M solution of HCl is added to a solution containing 0.150 moles of sodium phosphate (Na3PO4). The resulting solution is then diluted to exactly 1.00 L, at which time the pH was found to be pH 8.00. What is the concentration of H2PO4- in the solution? For phosphoric acid, Ka1 = 7.11 x 10-3, Ka2 = 6.32 x 10-8, and Ka3 = 7.1 X 10-13.
-What is the boiling point in oC of a 0.30 M solution of NaHSO4 if the solution has a density of 1.002 g/mL. Ka for hydrogen sulfate ion is 1.2 x 10–2?
What is the boiling point in oC of a 0.30 M solution of NaHSO4 if the solution has a density of 1.002 g/mL. Ka for hydrogen sulfate ion is 1.2 x 10–2.
A diprotic acid, H2A, has acid dissociation constants of
Ka1=1.01×10−4 and Ka2=4.08×10−12. Calculate the pH and molar
concentrations of H2A, HA−, and A2−at equilibrium for each of the
solutions.
A diprotic acid, H, A, has acid dissociation constants of Kal = 1.01 x 104 and K22 = 4.08 x 10-12. Calculate the pH and molar concentrations of H, A, HA, and A? at equilibrium for each of the solutions. A 0.176 M solution of H, A. pH= pH = 1...