A 25.00 mL sample of 0.300 M KOH analyte was titrated with 0.750 M HI at...

Question

Question

A 25.00 mL sample of 0.300 M KOH analyte was titrated with 0.750 M HI at 25 °C. Calculate the initial pH before any titrant w

science chemistry

Answer 1

Answer #1

initial pit before [ kolt}[OH-] = 0.3M polt= -log [ott] = -log (0-3)= 0.52288 plt=14-pott = 14-0.52288 = 13-477 kolt: molarit

Answer 2

Similar Homework Help Questions

A 25.00 mL sample of 0.280 M LiOH is titrated with 0.750 M HI at 25...

A 25.00 mL sample of 0.280 M LiOH is titrated with 0.750 M HI at 25 °C. Calculate the initial pH before any titrant is added. pH = Calculate the pH of the solution after 5.00 mL of the titrant is added. pH =
A 25.00 mL sample of 0.310 M NaOH is titrated with 0.750 M HCl at 25...

A 25.00 mL sample of 0.310 M NaOH is titrated with 0.750 M HCl at 25 °C. Calculate the initial pH before any titrant is added. Calculate the pH of the solution after 5.00 mL of the titrant is added.
A 25.00 mL sample of 0.280 M LiOH is titrated with 0.750 M HI at 25...

A 25.00 mL sample of 0.280 M LiOH is titrated with 0.750 M HI at 25 °C. initial ph = 13.45 calculate the ph after addition of 5.00 ml titrant is added.

3. A 25.00 mL sample of 0.200 M nitrous acid is titrated with 0.300 M sodium...

3. A 25.00 mL sample of 0.200 M nitrous acid is titrated with 0.300 M sodium hydroxide What is the pH of the solution when 10.00 mL of based has been added (K, = 4.6 x 104 for HNO.) 25 pts)
ration 46. A 30.0-ml sample of 0.165 M propanoic acid is titrated with 0.300 M KOH....

ration 46. A 30.0-ml sample of 0.165 M propanoic acid is titrated with 0.300 M KOH. Calculate the pH at each volume of added base: OmL, 5 mL, 10 mL, equivalence point, one-half equivalence point. 20 mL, 25 mL. Use your calculations to make a sketch of the titration curve. ed by
A.) A 20.0 mL sample of 0.0600 M carbonic acid (H2CO3) is titrated with 5.00 mL of 0.0960 M KOH...

A.) A 20.0 mL sample of 0.0600 M carbonic acid (H2CO3) is titrated with 5.00 mL of 0.0960 M KOH. What is the solution pH to the nearest hundredths place? pKa1 = 6.35 and pKa2 = 10.33. B.) A 20.0 mL sample of 0.0600 M carbonic acid (H2CO3) is titrated with 0.0960 M KOH. How many mL of titrant are required to reach the first equivalence point? C. )A 20.0 mL sample of 0.0600 M carbonic acid (H2CO3) is titrated...

A 50.0 mL solution of 0.150 M KOH is titrated with 0.300 M HCl. Calculate the...

A 50.0 mL solution of 0.150 M KOH is titrated with 0.300 M HCl. Calculate the pH of the solution after the addition of the following amounts of HCl. d) 18.0 mL HCl e) 24.0 mL HCl g) 26.0 mL HCl h) 29.0 mL HCl
25.00 mL of 0.218 M HBr is to be titrated with 0.199 M KOH. What is...

25.00 mL of 0.218 M HBr is to be titrated with 0.199 M KOH. What is the pH of the HBr solution after the addition of 55.8 mL of KOH? Report your answers to three decimal places.
- A40.0 mL. solution of 0.600 M Cu' in 1 M HNO was t titrated with...

- A40.0 mL. solution of 0.600 M Cu' in 1 M HNO was t titrated with 0.400 M Cef to give Cu and Ce The saturated calomel electrode was the reference e lectrode. (a) Write down the BALANCED titration reaction (b) Determine the equivalence volume. (c) Write the analyte half-reaction for the indicator electrode. (d) Write the titrant half-reaction for the indicator electrode (e) Write the analyte Nernst equation for the net cell reaction. (t) Write the titrant Nernst equation...

A 150 mL sample of a 0.300 M solution of K2SO3 is titrated with a 1.00 M HCl solution. Ka1=1.39E10^-2, Ka2=6.73E10^-8 Wh...

A 150 mL sample of a 0.300 M solution of K2SO3 is titrated with a 1.00 M HCl solution. Ka1=1.39E10^-2, Ka2=6.73E10^-8 What is the initial pH (before titration) and the pH after 50.0 mL of the 1.00 M HCl has been added?