# What is the Correct pH at the Endpoint of a Weak Acid Neutralization?

• pakmingki
In summary, an unknown quantity of weak acid HA was dissolved into water and 1 mL of 5 M NaOH was needed to neutralize it. The Ka of the acid is 3.2 x10^-4 and the pH at the endpoint is 8.30103.
pakmingki

## Homework Statement

You dissolve an unknown quantity of weak acid HA into 50 mL of water. It only takes 1 mL of 5 M NaOH to completely neutralize the acid. The Ka of the acid is 3.2 x10^-4. What is the pH at the endpoint?

## Homework Equations

Ka * Kb = Kw
pH + pOH = 14
p(of whatever) = -log(of whatever)

## The Attempt at a Solution

Ok, first, we know only 1 mL of 5 M NaOH was used. So, that means there were only 5mol NaOH/L * 1mol OH/1mol NaOH * 1 mL * 1L/1000mL which gives us 0.005 mol of OH were used. If 0.005 mol of OH was used, that means 0.005 mol of HA was neutralized.
Now, this is where i got messed up.
The principle reaction of this system is HA + OH = A + H20
If 0.005 mol of HA was neutralized by the HA, that means 0.005 mol of the A ion remains. We also know that A will ionize in the H20, so let's rewrite the formula. A + H20 = HA + OH
where there are initially 0.005 mols of A. We know for a fact all of those mols will not ionize to form 0.005 mol of HA, because since it's the conjugate base of a weak acid, it will not go all the way to the other side. So, we use Kb to determine the extent of the reaction. We are given Ka, and we know the relationship Ka * Kb = 1 x 10^-14.
Solving for Kb, we get 3.125 x 10^-11. In order to use the Kb relation, we need molarity instead of number of mols. Well, we know that there are 0.005 mol of A dissolved in 50 mL of water, so that gives us an initial molarity (before the reaction starts) of 0.1 M. We know that at equilibrium, there will be X M of OH and HA, so molarity of A at equilibrium is the initial molarity - molarity of OH, which is 0.1 - X. We can set the equation like any other reaction

Kb = ([OH][HA])/A
3.125 x 10^-11 = (x^2)/(0.1-x)
Solving for x which equals [OH], we get 2 x 10^-6.
Since we know [OH], we can find pOH which is -log[OH] = 5.69897
and we have the handy dandy formula pH + pOH = 14
pH = 14 - pOH = 8.30103

Now, i think i did the problem correctly, but i just have this feeling in my gut i did something wrong. Can someone run through my steps, or do the problem yourself and see if u get that answer?
This is a take home assignment, and i got to get good grades on the take home assignments. My entier grade in the class is based off of labs, take home assignments, and tests. Now, i can afford to screw up on tests and labs, because we can have retakes on tests, and my teacher let's us do lab corrections. But, there are no second chances on take home assignments.
thanks alot.

Last edited:
This is like asking what is the pH of the conjugate base of that weak acid. How many moles of HA was equivalent? What is the formality of the resulting NaA salt? You already have the Ka value, so take it from there.

One thing is definitely wrong. What is your FINAL volume?

At the endpoint you have solution of salt of weak acid. Check pH of weak acid salt lecture.

## 1. What is an acid base problem?

An acid base problem is a type of chemistry problem that involves calculating the pH or concentration of an acid or base solution. It also includes identifying the acid or base present in a solution.

## 2. How do I solve an acid base problem?

To solve an acid base problem, you will need to use the appropriate equations and formulas, such as the Henderson-Hasselbalch equation or the pH = -log[H+] equation. You will also need to know the properties of acids and bases, such as their strengths and dissociation constants.

## 3. What are some common mistakes when solving acid base problems?

Some common mistakes when solving acid base problems include forgetting to account for dilution, not considering the ionization of water, and not using the correct units. It is important to double-check your calculations and make sure you are using the correct formulas and units.

## 4. How can I check if my answer is correct?

You can check your answer by comparing it to the expected pH or concentration range for the given acid or base solution. You can also use an online pH calculator or ask a classmate or teacher to review your work.

## 5. What are some tips for solving acid base problems?

Some tips for solving acid base problems include making sure you understand the problem and what is being asked, using a systematic approach to solving the problem, and practicing with different types of acid base problems. It is also helpful to review the properties of acids and bases and the equations and formulas used to solve these types of problems.

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