Normal 0 false false false EN-US JA X-NONE /* Style Definitions */table.MsoNormalTable{mso-style-name:"Table Normal";mso-tstyle-rowband-size:0;mso-tstyle-colband-size:0;mso-style-noshow:yes;mso-style-priority:99;mso-style-parent:"";mso-padding-alt:0in 5.4pt 0in 5.4pt;mso-para-margin:0in;mso-para-margin-bottom:.0001pt;mso-pagination:widow-orphan;font-size:10.0pt;font-family:Cambria;} Calculate the pCN from the titration of 40.0 mL of 0.060 M NaCN with 20.0 mL of 0.050 M AgC 2 H 3 O 2 . The solubility product constant of AgCN is 2.2 x 10 -16 .

So here we need to figure out the negative log of our cyanide ion or cn. Here it says calculate pcn from the titration of 40 ml of 0.060 molar sodium cyanide with 20 ml of 0.050 molar of silver acetate. The solubility product constant of silver cyanide is 2.2 times 10 to the negative 16. Alright. So this represents our analyte. It is being titrated with silver chloride. So we're going to say here, molarity of my analyte times volume of my analyte equals molarity of my titrant times volume of my titrant. So here, that's going to be point 060 molar times volume equals the molarity of my titrant times the volume of my titrant, which I don't know. Divide both sides now by 0.050 molar. So volume of my titrant equals, we need 48 ml's. So like the previous question up above, we haven't quite reached our equivalence point yet. We only have 20 ml's of my titrant. So I'll have excess of my analyte remaining. So we're gonna say here the concentration of my analyte, which is cyanide ion, equals the millimoles of cyanide ion left, well, initially minus the millimoles of my titrant which is silver ion divided by the total volume. So here, multiply these together to get your millimoles. So here, we're gonna get 2.4millimoles minus 1.0millimoles divided by 40 ml+20 ml. So that's gonna give me a concentration of 0.023 molar of cyanide ion. Now that we have that, we take the negative log and We'll have our PCN, which comes out to 1.63. Remember, in terms of these questions, it's first important to remember who's the analyte and who's the titrant. We have to determine the equivalence volume of our titrant. From there determine are you dealing with calculations before the equivalence point, after the equivalence point or at the equivalence point. Once you know that, you'll know which equations to utilize, Once you know that, you'll know which equations to utilize to find either the concentration or the negative log of your particular analyte.

15. Redox Titrations

Titrations and Titration Curves

Analytical Chemistry

15. Redox Titrations

Titrations and Titration Curves

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Multiple Choice

Calculate the pCN from the titration of 40.0 mL of 0.060 M NaCN with 20.0 mL of 0.050 M AgC₂H₃O₂. The solubility product constant of AgCN is 2.2 x 10^-16.

1.53

0.023

1.45

1.63

0.029

Verified step by step guidance

Determine the initial moles of NaCN and AgC2H3O2. Use the formula: moles = concentration (M) × volume (L).

Write the balanced chemical equation for the reaction between NaCN and AgC2H3O2, which forms AgCN and NaC2H3O2.

Calculate the moles of AgCN formed using the stoichiometry of the reaction. Since the reaction is 1:1, the limiting reactant will determine the moles of AgCN formed.

Use the solubility product constant (Ksp) of AgCN to find the concentration of CN- ions in the solution. The Ksp expression for AgCN is: Ksp = [Ag+][CN-].

Calculate the pCN, which is the negative logarithm of the CN- concentration: pCN = -log[CN-].

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Struggling with Analytical Chemistry?

Calculate the pCN from the titration of 40.0 mL of 0.060 M NaCN with 20.0 mL of 0.050 M AgC2H­3O2. The solubility product constant of AgCN is 2.2 x 10-16.

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Titrations and Titration Curves practice set

Calculate the pCN from the titration of 40.0 mL of 0.060 M NaCN with 20.0 mL of 0.050 M AgC₂H₃O₂. The solubility product constant of AgCN is 2.2 x 10^-16.