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In a Strong Acid-Strong Base Titration we do not use an ICF Chart or ICE Chart to determine the pH of the solution. 

Strong Acid-Strong Base Titration

Concept #1: Strong Acid-Strong Base Titration

Example #1: Calculate the pH of the solution resulting from the titration of 75.0 mL of 0.100 M HBrO4 with 55.0 mL of 0.100 M NaNH2

Transcript

Let's take a look here where it says, 'Calculate the pH of the solution resulting from the titration of 75.0 mL of 0.100 M HBrO4 with 55 mL of 0.100 M NaNH2. Remember, this right here is a strong acid. This right here is a strong base. What we're going to say here is because both are strong, we don't have to use an ICE, we don’t have to use an ICF.
What do we do instead? We're going to say step one is find the moles. Remember, how do we find moles? Remember, moles equals molarity times liters. Divide the mL by a thousand, multiply them times their lit on their molarities.
Now, remember for the base, for the base you're always supposed to check how many OH minuses, NH2 minuses, H minuses and O2 minuses you have to get the correct concentration. Here we only have one NH2, so we don't have to worry about multiplying the concentration by anything, we can keep it as it is.
When we do this, we're going to say 0.075 L times 0.100 M HBrO4 equals 0.0075 M of HBrO4. Then we do the same thing with the other one, so we have that. Now that we found their moles, we're going to subtract the large one by the smaller one. What you're going to say is now you have this much left of your strong acid. That's all you're going to say, that's how much you have left of your strong acid.
Now step two, you're going to find molarity of whatever you have left. How do we find molarity? Well, we're going to take the moles that we just found and divide them by the total volume. Those two liters added up together will give you my total volume.
We're going to say 0.0020 moles of HBrO4 divide by the total volume we use, 0.0075 L plus 0.055 L. When we divide those together, that's going to give me, 0.0154 M HBrO4. Remember, since this is a strong acid, to find pH we don't need to do an ICE Chart. Since this is a strong acid, just take the negative log. Negative log of a strong acid will give me my pH.
So we plug in the concentration here and at the end, we scroll up some, at the end, what is that going to give me, my pH will be 1.81. So it's as simple as that. If both are strong, this is a great situation, first find the moles of both.
Remember look at the correct molarity of the strong base. If you have to multiply it by two because there's two OH or there's two NH2 or there's two Hs, H minuses, then you do that before you change everybody into moles.
Once you find moles, you subtract the larger moles from the smaller moles, whoever is left behind, whether it be a strong acid or a strong base, you immediately change it into molarity. If you have the molarity of a strong acid, take the negative log to find pH.
If you have the molarity of a base, so strong base then take the negative log of that, but that will give us pOH. So remember strong base if you take the negative log, it gives us pOH. If you have pOH, you're going to take that answer that you find and subtract it from 14 and that will give you pH. It's as simple as that.
Just remember the steps. Step one—find moles, step two—find molarity, step three—I guess you just take the negative log or whatever your answer is to find neither, pH or pOH. That's all you really have to do, there's no need of any type of chart.
Now that we've done this one, I want you guys to attempt to do the next one on your own as practice. So just take the same method that we used above in order to find it. Make sure that you get the correct concentrations of everyone before change everyone into moles. As long as you can remember that, you'll be able to solve this question. Good luck, guys. 

If after the titration there is an excess of strong acid left then we can use its concentration to find the pH. 

If after the titration there is an excess of strong base then we can use its concentration to find pOH initially. 

Practice: Calculate the pH of the solution resulting from the mixing of 175.0 mL of 0.250 M HNO3 with 75.0 mL of 0.200M Ba(OH)2.

If there is an equal amount of moles for both the strong acid and strong base then the pH of the solution will be 7. 

A student is titrating 38.0 mL of 0.0358 M solution of HBr with a 0.0289 M KOH solution. Calculate the pH of the solution after the addition of 43.19 mL of the KOH solution. A. 2.53 B. 3.57 C. 12.46 D. 2.86 E. 1.78
Determine the pH of a solution created by mixing 95.0 mL of 0.200 M nitric acid, HNO3, with 320.0 mL of 0.078 M potassium hydroxide, KOH. A. 2.22 B. 12.16 C. 0.91 D. 11.78 E. 1.84
A 10. mL sample of 0.20 M chloric acid solution is required to neutralize 20. mL of sodium hydroxide solution, NaOH.  a. What is the molarity of the sodium hydroxide solution?       b. What is the molarity of the salt that forms?
A 10. mL sample of 0.20 M hydrochloric acid solution is required to neutralize 20. mL of barium hydroxide, Ba(OH)2 a. What is the molarity of the barium hydroxide solution?       b. What is the molarity of the salt that forms?
Calculate the pH of a solution resulting from the titration of 113.00 mL of 0.0442 M HCIO3 with 82.65 mL of 0.0624 M LiOH. A. 10.92 B. 3.08 c. 10.21 D. 10.54 E. 7.00
A flask contains 50.0 mL of a 0.000968 M solution of Hydrochloric acid, HCl. The acid is to be titrated against 0.0275 M Sodium hydroxide, NaOH. What is the pH of the acid in the flask before the addition of any NaOH? a. 1.32 b. 1.71 c. 3.01 d. 4.32 e. 1.56
Calculate the pH of a solution created by mixing 120.0 mL of 0.375 M Perchloric Acid, HClO4, with 360.0 mL of 0.125 M lithium hydroxide, LiOH. a. 7.000 b. 0.426 c. 13.100 d. 0.602 e. 13.398
Calculate the pH of the solution resulting from the addition of 32.0 mL of 0.220 M HClO4 to 76.0 mL of 0.170 M NaOH. 1. 12.89 2. 7.00 3. 1.26 4. 1.11 5. 13.23 6. 12.74  7. 0.77
A 100.0 mL sample of 0.18 M HBrO 3 is titrated with 0.27 M LiH. Determine the pH of the solution after the addition of 30.0 mL of LiH. A) 0.86 B) 1.21 C) 2.00 D) 1.12 E) 2.86
Initially 7.1 g of HCl (MM = 36.46) and 9.5 g of NaOH (MM = 40.00) is added to water making a solution that has a volume of 12.85 L. What is the pH of the solution? A. 1.82 B. 2.48 C. 7.00 D. 11.52 E. 12.27
In the titration of a strong acid with a strong base, how would you calculate these quantities?pH beyond the equivalence point
Consider the titration of a 25.6 -mL sample of 0.125 M RbOH with 0.110 M HCl. Determine each of the following.the initial pH
Consider the titration of a 25.6 -mL sample of 0.125 M RbOH with 0.110 M HCl. Determine each of the following.the pH at 5.1 mL of added acid
In the titration of a strong acid with a strong base, how would you calculate these quantities?pH at the equivalence point
Consider the titration of a 25.6 -mL sample of 0.125 M RbOH with 0.110 M HCl. Determine each of the following.the pH at the equivalence point
A 25.00 mL sample of 0.320 M NaOH analyte was titrated with 0.750 M HI at 25 °C. a) Calculate the initial pH before any titrant was added. b) Calculate the pH of the solution after 5.00 mL of the titrant was added.
Calculate the pH of the resulting solution if 29.0 mL of 0.290 M HCl (aq) is added to 39.0 mL of 0.290 M NaOH (aq).
a. Write a balanced neutralization reaction between H2SO4 and KOH in aqueous solution. Phases are optional.b. 0.850 L of 0.420 M H2SO4 is mixed with 0.800 L of 0.210 M KOH. What concentration of sulfuric acid remains after neutralization?
A 100.00 mL sample of 0.18 M HClO 4 is titrated with 0.27 M LiOH. Determine the pH of the solution after the addition of 66.67 mL of LiOH (this is the equivalence point).a. 13.03 b. 7.00c. 2.76 d. 0.97 e. 11.24
Hydrochloric acid (75.0 mL of 0.250 M) is added to 225.0 mL of 0.0550 M Ba(OH)  2 solution. What is the concentration of the excess H+ or OH– ions left in this solution?
A student mixes four reagents together, thinking that the solutions will neutralize each other. The solutions mixed together are 50.0 mL of 0.100 M hydrochloric acid, 100.0 mL of 0.200 M of nitric acid, 500.0 mL of 0.0100 M calcium hydroxide, and 200.0 mL of 0.100 M rubidium hydroxide. Is the resulting solution neutral? If not, calculate the concentration of excess H+ or OH– ions left in solution.
Calculate the pH of the resulting solution if 20.0 mL of 0.200 M HCl(aq) is added to: a. 30.0 mL of 0.200 M NaOH(aq) b. 10.0 mL of 0.300 M NaOH(aq)
Consider the titration of a 36.0 mL sample of 0.175 M  HBr with 0.205 M KOH. Determine each of the following:the pH after adding 5.0 mL of base beyond the equivalence point
Calculate the pH during the titration of 40.00 mL of 0.1000 M HCl with 0.1000 M NaOH solution after each of the following additions of base:(f) 40.10 mL
Calculate the pH during the titration of 40.00 mL of 0.1000 M HCl with 0.1000 M NaOH solution after each of the following additions of base:(d) 39.90 mL
Calculate the pH during the titration of 40.00 mL of 0.1000 M HCl with 0.1000 M NaOH solution after each of the following additions of base:(g) 50.00 mL
A 20.0-mL sample of 0.150 M  KOH is titrated with 0.125 M  HClO4 solution. Calculate the pH after the following volumes of acid have been added.20.0 mL of the acid
A 20.0-mL sample of 0.150 M  KOH is titrated with 0.125 M  HClO4 solution. Calculate the pH after the following volumes of acid have been added.23.0 mL of the acid
Consider the titration of 40.0 mL of 0.200 M HClO 4 by 0.100 M KOH. Calculate the pH of the resulting solution after the following volumes of KOH have been added.e. 100.0 mL
Consider the titration of 80.0 mL of 0.100 M Ba(OH) 2 by 0.400 M HCl. Calculate the pH of the resulting solution after the following volumes of HCl have been added.a. 0.0 mL
Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M HBr solution after each of the following additions of acid:(a) 0 mL
Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M HBr solution after each of the following additions of acid:(b) 15.00 mL
Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M HBr solution after each of the following additions of acid:(c) 29.00 mL
Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M HBr solution after each of the following additions of acid:(d) 29.90 mL
Consider the titration of a 36.0 mL sample of 0.175 M  HBr with 0.205 M KOH. Determine each of the following:the pH at the equivalence point
Hydrochloric acid (75.0 mL of 0.250 M) is added to 225.0 mL of 0.0550 M Ba(OH)  2 solution. What is the concentration of the excess H+ or OH- ions left in this solution?
A student mixes four reagents together, thinking that the solutions will neutralize each other. The solutions mixed together are 50.0 mL of 0.100 M hydrochloric acid, 100.0 mL of 0.200 M of nitric acid, 500.0 mL of 0.0100 M calcium hydroxide, and 200.0 mL of 0.100 M rubidium hydroxide. Did the acids and bases exactly neutralize each other? If not, calculate the concentration of excess H+ or OH- ions left in solution.
A 50.0-mL sample of 0.200 M sodium hydroxide is titrated with 0.200 M nitric acid.What is the pH of the solution as the equivalence point?
Calculate the pH during the titration of 40.00 mL of 0.1000 M HCl with 0.1000 M NaOH solution after each of the following additions of base:(e) 40.00 mL
A 20.0-mL sample of 0.150 M  KOH is titrated with 0.125 M  HClO4 solution. Calculate the pH after the following volumes of acid have been added.24.0 mL of the acid
Consider the titration of 40.0 mL of 0.200 M HClO 4 by 0.100 M KOH. Calculate the pH of the resulting solution after the following volumes of KOH have been added.d. 80.0 mL
Consider the titration of 80.0 mL of 0.100 M Ba(OH) 2 by 0.400 M HCl. Calculate the pH of the resulting solution after the following volumes of HCl have been added.b. 20.0 mL
Calculate the pH at the halfway point and at the equivalence point for each of the following titrations.c. 100.0 mL of 0.50 M HCl titrated by 0.25 M NaOH
Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M HBr solution after each of the following additions of acid:(e) 30.00 mL
Consider the titration of a 36.0 mL sample of 0.175 M  HBr with 0.205 M KOH. Determine each of the following:the pH at 11.1 mL of added base
A 50.0-mL sample of 0.200 M sodium hydroxide is titrated with 0.200 M nitric acid. Calculate the pH of the solution, after you add a total of 55.6 mL 0.200 M HNO3.
Calculate the pH during the titration of 40.00 mL of 0.1000 M HCl with 0.1000 M NaOH solution after each of the following additions of base:(a) 0 mL
Calculate the pH during the titration of 40.00 mL of 0.1000 M HCl with 0.1000 M NaOH solution after each of the following additions of base:(b) 25.00 mL
A 20.0-mL sample of 0.150 M  KOH is titrated with 0.125 M  HClO4 solution. Calculate the pH after the following volumes of acid have been added.26.0 mL of the acid
A 20.0-mL sample of 0.150 M  KOH is titrated with 0.125 M  HClO4 solution. Calculate the pH after the following volumes of acid have been added.31.0 mL of the acid
Consider the titration of 40.0 mL of 0.200 M HClO 4 by 0.100 M KOH. Calculate the pH of the resulting solution after the following volumes of KOH have been added.a. 0.0 mL
Consider the titration of 40.0 mL of 0.200 M HClO 4 by 0.100 M KOH. Calculate the pH of the resulting solution after the following volumes of KOH have been added.b. 10.0 mL
Consider the titration of 40.0 mL of 0.200 M HClO 4 by 0.100 M KOH. Calculate the pH of the resulting solution after the following volumes of KOH have been added.c. 40.0 mL
Consider the titration of 80.0 mL of 0.100 M Ba(OH) 2 by 0.400 M HCl. Calculate the pH of the resulting solution after the following volumes of HCl have been added.c. 30.0 mL
Consider the titration of 80.0 mL of 0.100 M Ba(OH) 2 by 0.400 M HCl. Calculate the pH of the resulting solution after the following volumes of HCl have been added.d. 40.0 mL
Consider the titration of 80.0 mL of 0.100 M Ba(OH) 2 by 0.400 M HCl. Calculate the pH of the resulting solution after the following volumes of HCl have been added.e. 80.0 mL
Calculate the pH after the addition of 0.0 mL, 4.0 mL, 8.0 mL, 12.5 mL, 20.0 mL, 24.0 mL, 24.5 mL, 25.0 mL, 26.0 mL, 28.0 mL, and 30.0 mL of the NaOH for the titration of 25.0 mL of 0.100 M HNO3 with 0.100 M NaOH. Plot the results of your calculations as pH versus milliliters of NaOH added.
A 20.0-mL sample of 0.125 M HNO3 is titrated with 0.150 M NaOH. Calculate the pH for at least five different points throughout the titration curve and make a sketch of the curve.
A 15.0-mL sample of 0.100 M Ba(OH)2 is titrated with 0.125 M HCl. Calculate the pH for different points throughout the titration curve and make a sketch of the curve.
Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M HBr solution after each of the following additions of acid:(f) 30.10 mL
Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M HBr solution after each of the following additions of acid:(g) 40.00 mL
Calculate the pH of the resulting solution if 20.0 mL of 0.200 M HCl(aq) is added to:a. 30.0 mL of 0.200 M NaOH(aq)b. 10.0 mL of 0.300 M NaOH(aq)
A solid sample of Zn(OH)2 is added to 0.310 L of 0.520 M aqueous HBr. The solution that remains is still acidic. It is then titrated with 0.520 M NaOH solution, and it takes 90.5 mL of the NaOH solution to reach the equivalence point.What mass of Zn(OH)2 was added to the HBr solution?
A 25.0 mL sample of 0.105 M HCl was titrated with 315 mL of NaOH. What is the concentration of the NaOH?
The titration of 42.35 mL of H2SO4 requires 21.17 mL of 0.5000 M NaOH for complete neutralization. Calculate the concentration of H2SO4.(A) 0.2499 M H2SO4 (B) 0.1250 M H2SO4 (C) 0.4998 M H2SO4 (D) 1.000 M H2SO4 (E) 0.36 M H2SO4
Write the balanced neutralization reaction between H2SO4 (sulfuric acid) and KOH (potassium hydroxide) in aqueous solution. Also find the concentration of sulfuric acid remaining after 0.150L of 0.470 M H2SO4 is mixed with 0.100L of 0.230 M KOH. 
What is the pH of a solution made by mixing 40.0 mL of 0.100 M HCl with 25.00 mL of 0.100 M KOH? Assume that the volumes of the solutions are additive.A) 0.64B) 1.64C) 12.36D) 13.36E) 10.00
Calculate the pH of the resulting solution if 35.0 mL of 0.350 M HCl(aq) is added toa) 25.0 mL of 0.450 M NaOH(aq)pH = _____b) 45.0 mL of 0.350 M NaOH(aq)pH = _____
Calculate the pH of the resulting solution if 28.0 mL of 0.280 M HCl(aq) is added to(a) 38.0 mL of 0.280 M NaOH(aq)pH =(b) 18.0 mL of 0.380 M NaOH(aq).pH =
Calculate the pH of the resulting solution if 27.0 ml of 0.270 M HCl is added toa) 32.0 ml of 0.270 M NaOH(aq)b) 37.0 ml of 0.320 M NaOH(aq)
A 25.0 mL sample of 0.723 M HCIO4 is titrated with a 0.27 M KOH solution. The H3O+ concentration after the addition of 80.0 mL of KOH is _____ M. a) 0.4b) 1x10-7c) 0.7d) 3x10-13e) 4x10-2
A patient is suspected of having low stomach acid, a condition known as hypochloridia. To determine whether the patient has this condition, her doctors take a 19.00 mL sample of her gastric juices and titrate the sample with 0.000452 M KOH. The gastric juice sample required 11.3 mL of the KOH titrant to neutralize it. Calculate the pH of the gastric juice sample. Assume the sample contained no ingested food or drink which might otherwise interfere with the titration. For the patient to be suffering from hypochloridia, the pH of the gastric juices from the stomach must be greater than pH 4. Does the patient have hypochloridia?          (a) No          (b) Yes          (c) Unable to determine
What is the molarity of a sulfuric acid solution if it requires 62.55 mL of 0.09918 M NaOH to completely neutralize 25.00 mL of the acid? H2SO4 (aq) + 2NaOH (aq) → Na2SO4 (aq) + 2H2O (l) Give your answer to 4 significant figures and DO NOT include the units.
What volume of 0.236 M H2SO4 is needed to react with 53.5 mL of 0.104 M NaOH? The equation is H2SO4 aq) + 2NaOH (aq) → Na2SO4 (aq) + 2H2O (l) 
An aqueous solution of hydrobromic acid is standardized by titration with a 0.162 M solution of calcium hydroxide.If 21.5 mL of base are required to neutralize 27.6 mL of the acid, what is the molarity of the hydrobromic acid solution? 
Write the balanced neutralization reaction between H2SO4 and KOH in aqueous solution. Phases are optional. 0.750 L of 0.450 M H2SO4 is mixed with 0.700 L of 0.230 M KOH. What concentration of sulfuric acid remains after neutralization? 
How many moles of H3O+ or OH- must you add to a liter of strong base solution to adjust its pH from 8.090 to 7.720? Assume a negligible volume change.
Enter your answer in the provided box.If 46.01 mL of a standard 0.2577 M NaOH solution is required to neutralize 41.09 mL of H2SO4, what is the molarity of the acid solution?
100. mL of 0.200 M HCl is titrated with 0.250 M NaOH.i) What is the pH of the solution after 50.0 mL of base has been added? Express the pH numerically.    ii) What is the pH of the solution at the equivalence point? Express the pH numerically.
Consider the titration of 100.0 mL of 0.100 M NaOH with 1.00 M HBr. Find the pH at the following volumes of acid added: 0, 5,10,12 mL