A 50.0ml aliquot of 0.100 M NaOH is titrated with 0.200 M HCl. Calculate the pH...

A 50.0ml aliquot of 0.100 M NaOH is titrated with 0.200 M HCl. Calculate the pH of the solution after addition of 0.0, 5.0, 10.0, 25.0, 35.0, 45.0, 55.0 of HCl. Plot the titration curve in a graph paper.

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queen_honey_blossom answered 1 year ago

A 25 mL aliquot of an HCl solution is titrated with 0.100 M NaOH. The equivalence...

A 25 mL aliquot of an HCl solution is titrated with 0.100 M NaOH. The equivalence point is reached after 21.27 mL of the base were added. Calculate 1) the concentration of the acid in the original solution, 2) the pH of the original HCl solution and the original NaOH solution, 3) the pH after 10.00 mL of NaOH have been added, 4) the pH at the equivalence point, and 5) the pH after 25.00 mL of NaOH have been...

When 50.0mL of 0.100 M NaOH and 50.0mL of 0.100 M HCL are mixed. what is...

When 50.0mL of 0.100 M NaOH and 50.0mL of 0.100 M HCL are mixed. what is the pH of the resultant solution? (show two chemical equations to obtain [H+] and then calculate pH)

A 40.0 mL sample of 0.100 M HCl is titrated with 0.100 M NaOH. Calculate the...

A 40.0 mL sample of 0.100 M HCl is titrated with 0.100 M NaOH. Calculate the pH after the addition of each of the following volumes of NaOH: (a) 0.0 mL, (b) 10.0 mL, (c) 20.0 mL, (d) 40.0 mL, (e) 60.0 mL. A plot of the pH of the solution as a function of the volume of added titrant is known as a pH titration curve. Using the available data points, plot the pH titration curve for the above...

25.00 mL 0.100 M CH3NH2 is titrated with 0.100 M HCl. Calculate the pH of this...

25.00 mL 0.100 M CH3NH2 is titrated with 0.100 M HCl. Calculate the pH of this the titration solution after the addition of a) 12.5 mL and b) 25.00 mL of the titrant has been added. Based on these pH values, select an appropriate indicator for the titration from table at the end of lecture notes for Chapter 16.

30.0 mL of 0.100 M H2CO3 is titrated with 0.200 M KOH. Calculate the initial pH...

30.0 mL of 0.100 M H2CO3 is titrated with 0.200 M KOH. Calculate the initial pH before KOH has been added. ka = 4.3 x 10-7. Calculate the pH when 10.0 mL of a .200M KOH is added to 30.0 mL of 0.100 M H2CO3. ka = 4.3 x 10-7. Calculate the equivalence point and then calculate the pH at the equivalence point. Calculate the pH if 20.0 mL of 0.200 M KOH is added to 30.0 mL of 0.100...

50.0ml of 0.125M HF is titrated with 0.100M NaOH. Calculate the pH after the addition of...

50.0ml of 0.125M HF is titrated with 0.100M NaOH. Calculate the pH after the addition of a) 0.00ml of NaOH b) 15.00ml of NaOH c) 31.25ml of NaOH d) 60.00ml of NaOH e) 62.50ml of NaOH f) 70.00ml of NaOH

A25.0 mL sample of 0.100 M NaOH is titrated with a 0.100 M HNO3 solution. Calculate...

A25.0 mL sample of 0.100 M NaOH is titrated with a 0.100 M HNO3 solution. Calculate the pH after the addition of 0.0, 4.0, 8.0, 12.5, 20.0, 24.0, 24.5, 24.9, 25.0, 25.1, 26.0, 28.0, and 30.0 of the HNO3.

A 25.0−mL solution of 0.100 M CH3COOH is titrated with a 0.200 M KOH solution. Calculate...

A 25.0−mL solution of 0.100 M CH3COOH is titrated with a 0.200 M KOH solution. Calculate the pH after the following additions of the KOH solution (a) 10.0 mL (b) 12.5 mL (c) 15.0 mL

A 40.0-mL sample of 0.100 M HNO2 is titrated with 0.200 M KOH. Calculate: a.the volume...

A 40.0-mL sample of 0.100 M HNO2 is titrated with 0.200 M KOH. Calculate: a.the volume required to reach the equivalence point b.the pH after adding 15.00 mL of KOH c.the pH at one-half the equivalence point

Pertaining to the titration of 25.0mL of 0.100 M HCN (Ka=6.2x10-10) with 0.200 M NaOH, calculate...

Pertaining to the titration of 25.0mL of 0.100 M HCN (Ka=6.2x10-10) with 0.200 M NaOH, calculate the pH at the following points. a) initial pH, 0.0mL NaOH b) after the addition of 4.0mL NaOH c) after the addition of 6.25 mL NaOH d) at the equivalence point e) after the addition of 17.0 mL NaOH

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