The base hydrolysis constant (Kb) for benzoate ion (C7H5O2 - ,“A-”) is 1.6 × 10-10
150.00 mL of 0.20 M HCl was added to 100.00-mL sample of 0.25 M NaC7H5O2. Calculate the pH of the resulting solution
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The base hydrolysis constant (Kb) for benzoate ion (C7H5O2 - ,“A-”) is 1.6 × 10-10 150.00...
Sodium benzoate (NaC7H5O2, “NaA”) is a weak base. The base hydrolysis constant (Kb) for benzoate ion (C7H5O2 - , “A- ”) is 1.6 × 10-10. (1) What is the pH of a 0.25 M NaC7H5O2 aqueous solution? Show work please! (2) During a titration, 40.00 mL of 0.20 M HCl was added to 100.00-mL sample of 0.25 M NaC7H5O2. Calculate the pH of the resulting solution. Show work please!
Sodium benzoate (NaC7H5O2, “NaA”) is a weak base that is commonly used as a food preservative. The base hydrolysis constant (Kb) for benzoate ion (C7H5O2 - , “A- ”) is 1.6 × 10-10. (a) What is the pH of a 0.25 M NaC7H5O2 aqueous solution? Show work
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Sodium benzoate (NaC7H5O2) is sometimes used as a preservative in foods. Benzoic acid is the conjugate acid of the benzoate ion, which has a Ka value of 6.3 x 10-5. Calculate the Kb value for the benzoate ion. (1 mark) Use the Kb value for the benzoate ion from part a, calculate the pH of a 0.215 M solution of the sodium benzoate. (Ignore x method, 4 marks)
NH3 is a weak base with a Kb value of 1.76x10–5. Suppose 25.0 mL of a0.180 MNH3 is titrate using HCl. The end point is reach after 35.0 mL HCl had been added. Calculate the pH of the resulting solution at the equivalence-point. Here is the titration equation:NH3(aq) + HCl(aq) →NH4Cl(aq)
A weak base has Kb =
. Calculate the hydrolysis constant, Ka, for the weak conjugate
acid.
7.7.c10-10 A weak base has Kp = 7.7 x 10–10. Calculate the hydrolysis constant, Ka, for the weak conjugate acid. Ka=
Question about ACID/BASE. Equal volumes of 0.230 M weak base (Kb = 4.0× 10–9) and 0.230 M HCl are mixed. Calculate the pH of the resulting solution. Please show all your work.
You have 40.00 mL of a 0.300 M aqueous solution of the weak base C6H5NH2 (Kb = 4.00 x 10-10). This solution will be titrated with 0.300 M HCl. (a) How many mL of acid must be added to reach the equivalence point? (b) What is the pH of the solution before any acid is added? (c) What is the pH of the solution after 10.00 mL of acid has been added? (d) What is the pH of the solution...