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(2 points) A 50.0 mL solution of 0.040 M pyridine (C6HSN) was titrated with 0.0500 M...
A 40.0 mL volume of 0.100 M NaOH is titrated with 0.0500 M HCl. Calculate the pH after addition of the following volumes of acid. A). 83.6 mL
A 98.0 mL sample of 0.0500 M HBr is titrated with 0.100 M CSOH solution. Calculate the pH after the following volumes of base have been added. (a) 14.2 mL (b) 47.5 mL (c) 49.0 mL pH = pH = pH (d) 51.0 mL (e) 80.4 mL pH = pH =
Consider the titration of 50.0 mL of 0.0500 M H2NNH2 (a weak base; Kb = 1.30e-06) with 0.100 M HIO4. Calculate the pH after the following volumes of titrant have been added: (a) 0.0 mL (b) 6.3 mL (c) 12.5 mL pH = DHO pH = (d) 18.8 ml (e) 25.0 ml (0) 37.5 mL pH = 0 pH = pH -
The dibasic compound B (pKb1 5 4.00, pKb2 5 8.00) was titrated with 1.00 M HCl. The initial solution of B was 0.100 M and had a volume of 100.0 mL. Find the pH at the following volumes of acid added and make a graph of pH versus Va: Va 5 0, 1, 5, 9, 10, 11, 15, 19, 20, and 22 mL. pKb1= 4.00 pkb2= 8.00 11-23. The dibasic compound B (pKb1 = 4.00, pKb2 = 8.00) was titrated...
6. (8) A 50.0 mL sample of hard water containing Ca2 was titrated with 0.0500 M EDTA standard solution at pH 10 and with Eriochrome Black T indicator. The endpoint was reached when 11.35 mL of EDTA was added a) (6) Calculate the concentration of Ca* in the unknown sample in moles per liter (M). b) (2) What is the pCa of the solution?
25. A 50.0 mL sample of 0.150 M weak acid was titrated with a 0,150 M NaOH solution. What is the pH after 30.0 mL of the sodium hydroxide solution is added? The Ka of the acid is 1.9x10(3 points) D) 4.78 E) None of these C) 3.03 (A) 4.90 B) 1.34 26. A 25.0 mL sample of 0.25 M hydrofluoric acid (HF) is titrated with a 0.25 M NaOH solution. What is the pH after 38.0 mL of base...
2. (5 Points) 25.00 mL of 0.0750 M sodium benzoate (NaC6H3CO2) is titrated with 0.100 M HCl. Find the pH of the solution for the following volumes of acid added: 0 mL, 1 mL, 5 mL, 10 mL, 15 mL, 17 mL, 18 mL, 18.75 mL, 20 mL, 22 mL, 25 ml, and 30 mL. Create a titration curve.
A 50.0 mL solution of 0.156 M KOH is titrated with 0.312 M HCl. Calculate the pH of the solution after the addition of each of the given amounts of HCI. 0.00 mL pH = 13.2 6.00 mL pH = 13.1 12.5 mL pH = 12.84 20.0 mL pH = 13.35 24.0 mL pH = 13.32 25.0 mL pH = 13.32 26.0 mL 200 mL o pH = pH = 12:37 30.0 mt p# = 12.40 12.37 30.0 mL pH...
a 50.0 mL sample of a 0.100 M solution of NaCN is titrated by 0.100 M HCl. kb for CN is 2.0x10-5. A.calculate the pH of the solution prior to the start of the titration. B after the addition of 10.0 mL. C. after the addition of 25.0 mL of 0.100 M HCl. D. at the equivalence point. E. after the addition of 60.0 mL of 0.100 M HCl
A 25.0-mL sample of a 0.250 M solution of aqueous trimethylamine is titrated with a 0.313 M solution of HCl. Calculate the pH of the solution after 10.0, 20.0. and 30.0 ml of acid have been added; pKb of (CH3)3N = 4.19 at 25degreeC. pH after 10.0 mL of acid have been added; 4.19 Number Did you find the pH or the pOH of this solution? pH after 20.0 mL of acid have been added: Number 3.65 pH after 30.0...