Problem: A mixture of NaCN and NaHSO4 consists of a total of 0.60 mol. When the mixture is dissolved in 1.0 L of water and comes to equilibrium the pH is found to be 9.6.Find the amount of NaCN in the mixture.

🤓 Based on our data, we think this question is relevant for Professor Billman's class at Abilene Christian University.

FREE Expert Solution

We are asked to calculate the amount of NaCN in a mixture of NaCN and NaHSOconsisting of a total of 0.60 mol. When the mixture is dissolved in 1.0 L of water and comes to equilibrium the pH is found to be 9.6.

NaCN and NaHSO4  are both ionic compounds of sodium with conjugate bases of weak acid CN- and strong acid HSO4-


The dissociation of NaCN and NaHSOare as follows:

NaCN (aq) → Na+ (aq) + CN- (aq)

NaHSO4(aq) →  Na+(aq) + HSO4-(aq)

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Problem Details

A mixture of NaCN and NaHSO4 consists of a total of 0.60 mol. When the mixture is dissolved in 1.0 L of water and comes to equilibrium the pH is found to be 9.6.

Find the amount of NaCN in the mixture.

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Diprotic Acid concept. You can view video lessons to learn Diprotic Acid. Or if you need more Diprotic Acid practice, you can also practice Diprotic Acid practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Billman's class at Abilene Christian University.