Here we’ll go over an example where a strong acid is mixed with a strong base, and we calculate the pH of the final mixture. Strong Acid–Strong Base Mixture.

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Presentation transcript:

Here we’ll go over an example where a strong acid is mixed with a strong base, and we calculate the pH of the final mixture. Strong Acid–Strong Base Mixture Calculations Example 1

We’re given that mL of M Sr(OH) 2 is added to mL of M HNO mL of M Sr(OH) 2 is added to mL of M HNO 3.

And we’re asked to calculate the pH of the final mixture mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture.

We’ll point out something important here. Strontium hydroxide is a strong base, mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture.

and its formula, Sr(OH)2, has 2 OH’s in it mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture.

So when we write the balanced dissociation equation for Sr(OH) mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture. Dissociation Equation

We see that there are 2 moles of OH- for each mole of Sr(OH) mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture. A conversion factor

So we can use this as a conversion factor mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture. A conversion factor

We’ll start by calculating the initial moles of OH minus added mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture.

We take moles of Sr(OH)2 per L mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture.

Multiply it by the conversion factor 2 mol OH- over 1 mole Sr(OH) mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture.

And by L. We rounded this to 3 significant figures to save room here. The concentration mol/L is only 3 significant figures so the answer to this calculation is limited to 3 significant figures mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture.

When we multiply all three numbers we get mol. So the initial moles of OH minus added is mol. Notice, this is expressed to 3 significant figures, which is consistent with the given data mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture.

Our next step is to calculate the initial moles of H+ added mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture.

The H+ comes from the strong acid nitric acid, or HNO3. Each HNO3 releases 1 proton, so we take mol HNO3 per L mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture.

Times 1 mol of H+ per 1 mol of HNO mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture.

Times L. Again we rounded this to 3 significant figures to save room. The number of significant figures in the answer is limited by the 3 significant figures in M mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture.

The answer comes out to mol. So the initial moles of H+ added is moles mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture.

Notice that in preserving 3 significant figures, both of these have 4 decimal places mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture.

Comparing the initial moles of OH minus with the initial moles of H+, we see that we have more moles of OH minus than of H+, so the OH minus is in excess in this case mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture. Excess

The excess moles of OH minus mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture.

Is mol OH minus mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture.

minus mol H mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture.

Which equals mol OH minus mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture.

Notice the numbers we’re subtracting both have 4 decimal places, so our answer must also have 4 decimal places mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture. 4 decimal places

When expressed to 4 decimal places, this number has 3 significant figures. The zero’s to the left of the 2 are not significant, but the zero after the 5 is mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture. 3 significant figures

Since the hydroxide ion is in excess, we calculate its concentration in the final mixture. It is equal to mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture.

moles mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture.

Divided by the total volume of the solution, which is L of Strontium hydroxide solution, mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture.

Plus L of HNO3 solution mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture.

So the concentration of OH minus is moles over L mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture.

Which Equals molar mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture.

Because we have base in excess, we can calculate the pOH mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture.

Which is the negative log of the hydroxide ion concentration mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture.

Or the negative log of mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture.

Which comes out to None of our data or calculations in this problem have less than 3 significant figures, so the pOH has 3 significant figures or three decimal places mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture.

Now we can calculate the pH mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture.

Which is 14 minus the pOH mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture.

Or 14 minus mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture.

Which is This must has 3 significant figures so its expressed to 3 decimal places mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture.

We have now answered the question we set out to answer. The pH of the final mixture is This is relatively highly basic which is consistent with the fact that OH- is in excess. pH of final mixture mL of M Sr(OH) 2 is added to mL of M HNO 3. Calculate the pH of the final mixture.