Question

In: Chemistry

In the titration of 0.010 L of 2.0 M NaOH with 1.0 M HI, what is...

In the titration of 0.010 L of 2.0 M NaOH with 1.0 M HI, what is the pH when 0.015 L of HI have been added?

Expert Solution

HI NaOH

MA = 1M MB = 2M

VA = 0.015L VB = 0.010M

M = MBVB-MAVA/VA+VB MBVB>MAVA

= 2*0.010 -1*0.015/0.01+0.015

= 0.005/0.01+0.015

= 0.005/0.025 = 0.2 M

[OH^-] = M = 0.2M

POH = -log[OH^-]

= -log0.2

= 0.6989

PH = 14-POH

= 14-0.6989

= 13.3011 >>>>answer

= -log0.2

queen_honey_blossom answered 1 year ago

How many grams of NaOH must be added to 1.0 L of 2.0 M HC2H3O2 to...

How many grams of NaOH must be added to 1.0 L of 2.0 M HC2H3O2 to produce a buffer solution with a pH = 4.80. Ka = 1.8 × 10-5

What amount of solid NaOH must be added to 1.0 L of a 0.12 M H2CO3...

What amount of solid NaOH must be added to 1.0 L of a 0.12 M H2CO3 solution to produce a solution with [H+]= 3.0×10−11 M ? There is no significant volume change as the result of the addition of the solid.

Consider the titration of 50.5 mL of 1.1 M NaOH with 1.0 M HCl. You may...

Consider the titration of 50.5 mL of 1.1 M NaOH with 1.0 M HCl. You may want to reference ( pages 682 - 686) Section 16.9 while completing this problem. Part A What is the pH at the start of the titration? Express the pH to two decimal places. Part B What is the pH at the equivalence point? Express the pH to two decimal places. Part C What is the pH after the addition of a large excess of...

Consider the titration of 20 mL of 0.010 M V2+ with 0.010 M Fe3+ in 1...

Consider the titration of 20 mL of 0.010 M V2+ with 0.010 M Fe3+ in 1 M HCl using Pt and saturated calomel electrodes. Write a balanced titration reaction and the two half reactions for the indicator electrode. Calculate E at the following volumes of Fe3+ added: 1.00, 10.00, 20.00, and 30.00 mL

A student has a 1.0 L solution of 2.0 M HCl and wants to increase the...

A student has a 1.0 L solution of 2.0 M HCl and wants to increase the HCl concentration to 3.0 M. Which action will produce the intended outcome? A) Add 1.0 L of 4.0 M HCl to the existing solution B) Add 1.0 L of 1.0 M HCl to the existing solution C) Add 1.0 L of 3.0 M NaCl to the existing solution D) Add 1.0 L of 12 M HCl to the existing solution E) Add 1.0 L...

1. What quantity (moles) of NaOH must be added to 1.0 L of 2.1 M HC2H3O2...

1. What quantity (moles) of NaOH must be added to 1.0 L of 2.1 M HC2H3O2 to produce a solution buffered at pH = 4.00? Ka = 1.8×10-5 mol 2. What quantity (moles) of NaOH must be added to 1.0 L of 2.1 M HC2H3O2 to produce a solution buffered at pH = 5.00? Ka = 1.8×10-5 mol I really need help! Please show every step of the math no matter how small! Thank you

Consider the titration of 100.0 mL of 1.00 M HA (Ka=1.0*10^-6) with 2.00 M NaOH. A....

Consider the titration of 100.0 mL of 1.00 M HA (Ka=1.0*10^-6) with 2.00 M NaOH. A. Determine the pH before the titration begins B. Determine the volume of 2.00 M NaOH required to reach the equivalence point C. Determine the pH after a total of 25.0 mL of 2.00 M NaOH has been added D. Determine the pH at the equivalence point of the titration. Thank you in advance!

12. Consider the titration of 0.100 L of 0.200 M ascorbic acid with 0.500 M NaOH....

12. Consider the titration of 0.100 L of 0.200 M ascorbic acid with 0.500 M NaOH. What is the pH at the endpoint of the titration? Enter your answer to two decimal places; for this question we can assume the 5% assumption is valid.

what is the concentration of Cd2+ in a 0.010 M Cd(NO3)2 solution that is also 1.0...

what is the concentration of Cd2+ in a 0.010 M Cd(NO3)2 solution that is also 1.0 M NH3? For Cd(NH3)4^2+, Kf=1.0x10^7

1) Calculate the pH of 1.0 L of the solution upon addition of 0.010 mol of...

1) Calculate the pH of 1.0 L of the solution upon addition of 0.010 mol of solid NaOH to the original buffer solution. 2) Calculate the pH of 1.0 L of the solution upon addition of 30.0 mL of 1.0 MHCl to the original buffer solution. 3) A 1.0L buffer solution contains 0.100 molHC2H3O2 and 0.100 molNaC2H3O2. The value of Ka for HC2H3O2 is 1.8×10−5. 3A) Calculate the pH of the solution upon the addition of 0.015 mol of NaOH...