18. Aqueous Equilibrium

Strong Acid Strong Base Titrations

Titration of a strong acid with a strong base | Chemistry | Khan Academy

Two 25.0-mL samples, one 0.100 M HCl and the other
0.100 M HF, are titrated with 0.200 M KOH.
c. Which titration curve has the lower initial pH?

17.3a pH Calculations for Strong Acid Strong Base Titrations | General Chemistry

The probe of the pH meter shown here is sitting in a beaker
that contains a clear liquid. You are told the liquid is
pure water, a solution of HCl(aq), or a solution of KOH(aq). (b) If the liquid is one of the solutions,
what is its molarity?
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/36981dd1959937c5-1667230596615.jpg" alt="" />

Calculate the pH of a solution made by adding 2.50 g of 
lithium oxide 1Li2O2 to enough water to make 1.500 L of 
solution.

Consider the titration of a 35.0-mL sample of 0.175 M HBr with 
0.200 M KOH. Determine each quantity. 
c. the pH at 10.0 mL of added base

How many grams of CaO should be dissolved in sufficient 
water to make 1.00 L of a solution with a pH of 10.50?

The volume of an adult’s stomach ranges from about 50 
mL when empty to 1 L when full. If the stomach volume is 
400 mL and its contents have a pH of 2, how many moles 
of H+ does the stomach contain? Assuming that all the H+ 
comes from HCl, how many grams of sodium hydrogen 
carbonate will totally neutralize the stomach acid?

Calculate the concentration of an aqueous solution of Ca1OH22 that has a pH of 10.05.

For each strong base solution, determine [OH-], [H3O+], pH,
and pOH.
b. 1.5 * 10-3 M Ca(OH)2

Consider the titration of a 35.0-mL sample of 0.175 M HBr with
0.200 M KOH. Determine each quantity.
e. the pH after adding 5.0 mL of base beyond the equivalence
point

What is the pH of a solution in which 224 mL of HCl(g), measured 
at 27.2 °C and 1.02 atm, is dissolved in 1.5 L of aqueous solution?

For each strong base solution, determine [OH-], [H3O+], pH,
and pOH.
c. 1.9 * 10-4 M KOH

Consider the titration of a 35.0-mL sample of 0.175 M HBr with
0.200 M KOH. Determine each quantity.
a. the initial pH

Two 20.0-mL samples, one 0.200 M KOH and the other 
0.200 M CH3NH2, are titrated with 0.100 M HI. 
b. Is the pH at the equivalence point for each titration acidic, 
basic, or neutral?

What is the pH at the equivalence point for the titration of 0.20 M solutions of the following acids and bases? Which of the indicators in Figure 17.5 would be suitable for each titration? 
(c) Ba(OH)2 and HBr<img src="https://lightcat-files.s3.amazonaws.com/problem_images/f4855ca73f1676bb-1673291984591.jpg" alt="" />

If after the titration there is an excess of strong base then we can use its concentration to find pOH initially.&#160;

Determine the pH of each two-component solution.
d. 0.088 M HClO4 and 0.022 M KOH

For each strong acid solution, determine [H3O+], [OH-], and pH.
d. a solution that is 0.655% HNO3 by mass (assume a density of
1.01 g>mL for the solution)

Calculate the pH of solutions prepared by: 
(a) Dissolving 0.20 g of sodium oxide in water to give 
100.0 mL of solution.

If the following solutions are mixed, is the resulting solution acidic, basic, or neutral?
(a) 50.0 mL of 0.100 M HBr and 30.0 mL of 0.200 M KOH

Calculate the pH of solutions prepared by:
(a) Dissolving 4.8 g of lithium hydroxide in water to give
250 mL of solution.

Two 20.0-mL samples, one 0.200 M KOH and the other
0.200 M CH3NH2, are titrated with 0.100 M HI.
a. What is the volume of added acid at the equivalence point
for each titration?

If after the titration there is an excess of strong acid left then we can use its concentration to find the pH.&#160;

For each strong base solution, determine [OH-], [H3O+], pH,
and pOH.
b. 0.0112 M Ba(OH)2

Calculate the pH of the following solutions: 
(c) 0.075 M NaOH

For each strong base solution, determine [OH-], [H3O+], pH,
and pOH.
a. 8.77 * 10-3 M LiOH

A solid sample of Fe1OH23 is added to 0.500 L of 0.250 M
aqueous H2SO4. The solution that remains is still acidic. It
is then titrated with 0.500 M NaOH solution, and it takes
12.5 mL of the NaOH solution to reach the equivalence
point. What mass of Fe1OH23 was added to the H2SO4
solution?

How many milliliters of 0.0850 M NaOH are required to 
titrate each of the following solutions to the equivalence 
point: (c) 50.0 mL of a solution that contains 
1.85 g of HCl per liter?

Two 25.0-mL samples, one 0.100 M HCl and the other
0.100 M HF, are titrated with 0.200 M KOH.
b. Is the pH at the equivalence point for each titration acidic,
basic, or neutral?

Calculate 3OH-4 and pH for each of the following strong base solutions: (c) 10.0 mL of 0.0105 M Ca1OH22 diluted to 500.0 mL

Make a rough plot of pH versus milliliters of acid added for the titration of 50.0 mL of 1.0 M NaOH with 1.0 M HCl. Indicate the pH at the following points, and tell how many milliliters of acid are required to reach the equivalence point. 
(a) At the start of the titration
(b) At the equivalence point 
(c) After the addition of a large excess of acid

Calculate the pH of each of the following strong acid solutions:
(b) 1.52 g of HNO3 in 575 mL of solution

Calculate the pH of each of the following strong acid solutions:
(b) 0.225 g of HClO3 in 2.00 L of solution

pH in Strong Acid-Strong Base Titrations

Strong Acid-Strong Base Titration

For each strong acid solution, determine [H3O+], [OH-], and pH.
b. 0.015 M HNO3

Consider the titration of a 35.0-mL sample of 0.175 M HBr with 
0.200 M KOH. Determine each quantity. 
b. the volume of added base required to reach the equivalence 
point

A 100.0 mL sample of a solution that is 0.100 M in HCl 
and 0.100 M in HCN is titrated with 0.100 M NaOH. Calculate 
the pH after the addition of the following volumes of 
NaOH: 
(b) 75.0 mL

Consider the titration of a 25.0-mL sample of 0.115 M RbOH
with 0.100 M HCl. Determine each quantity.
b. the volume of added acid required to reach the equivalence
point

Calculate the pH of solutions prepared by: 
(d) Mixing 100.0 mL of 2.0 * 10-3 M HCl and 400.0 mL of 
1.0 * 10-3 M HClO4. (Assume that volumes are additive.)

People often take milk of magnesia to reduce the discomfort associated
with acid stomach or heartburn. The recommended
dose is 1 teaspoon, which contains 4.00 * 102 mg of Mg(OH)2.
What volume of an HCl solution with a pH of 1.3 can be neutralized
by one dose of milk of magnesia? If the stomach contains 2.00 * 102 mL of pH 1.3 solution, is all the acid neutralized? If not, what fraction is neutralized?

Strong Acid-Strong Base

Two 20.0-mL samples, one 0.200 M KOH and the other
0.200 M CH3NH2, are titrated with 0.100 M HI.
c. Which titration curve has the lower initial pH?

A 20.0-mL sample of 0.200 M HBr solution is titrated with 
0.200 M NaOH solution. Calculate the pH of the solution 
after the following volumes of base have been added: 
(e) 35.0 mL.

A solution is made by adding 0.300 g Ca1OH221s2, 50.0 mL of 1.40 M HNO3, and enough water to make a final volume of 75.0 mL. Assuming that all of the solid dissolves, what is the pH of the final solution?

What mass of HClO4 must be present in 0.500 L of solution to
obtain a solution with each pH value?
b. pH = 1.50

Lakes that have been acidified by acid rain can be neutralized by 
liming, the addition of limestone (CaCO3). How much limestone 
(in kg) is required to completely neutralize a 4.3 billion 
liter lake with a pH of 5.5?

Titration of a strong acid with a strong base (continued) | Chemistry | Khan Academy

Strong Acid / Strong Base Titration Curve - All pH Calculations

For each strong acid solution, determine [H3O+], [OH-], and pH.
a. 0.25 M HCl

Strong acid–strong base titrations | Acids and bases | AP Chemistry | Khan Academy

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: (c) 24.0 mL.

For each strong acid solution, determine [H3O+], [OH-], and pH.
c. a solution that is 0.052 M in HBr and 0.020 M in HNO3

Calculate the pH at the equivalence point in titrating 0.100 
M solutions of each of the following with 0.080 M NaOH: 
(a) hydrobromic acid (HBr).

(a) What volume of 0.115 M HClO4 solution is needed to
neutralize 50.00 mL of 0.0875 M NaOH?

Consider the titration of a 25.0-mL sample of 0.115 M RbOH 
with 0.100 M HCl. Determine each quantity. 
c. the pH at 5.0 mL of added acid

What is the pH of an aqueous solution of Ca1OH22 at 25.0 °C 
with a concentration of 6.3 * 10-5 M? (LO 16.7) 
(a) 4.20 (b) 10.10 
(c) 11.36 (d) 9.80

17.2 Titrations and Titration Curves | General Chemistry

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.&#160;

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.

Consider the titration of 60.0 mL of 0.150 M HNO3 with 0.450 M NaOH.
(a) How many millimoles of HNO3 are present at the start of the titration?
(b) How many milliliters of NaOH are required to reach the equivalence point?
(c) What is the pH at the equivalence point? 
(d) Sketch the general shape of the pH titration curve.

Consider the titration of a 35.0-mL sample of 0.175 M HBr with
0.200 M KOH. Determine each quantity.
d. the pH at the equivalence point

Determine the pH of a solution that is 3.85% KOH by mass. 
Assume that the solution has density of 1.01 g>mL.

For each strong base solution, determine [OH-], [H3O+], pH,
and pOH.
d. 5.0 * 10-4 M Ca(OH)2

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Chad's Prep

1. Intro to General Chemistry

2. Atoms & Elements

3. Chemical Reactions

4. BONUS: Lab Techniques and Procedures

5. BONUS: Mathematical Operations and Functions

6. Chemical Quantities & Aqueous Reactions

7. Gases

8. Thermochemistry

9. Quantum Mechanics

10. Periodic Properties of the Elements

11. Bonding & Molecular Structure

12. Molecular Shapes & Valence Bond Theory

13. Liquids, Solids & Intermolecular Forces

14. Solutions

15. Chemical Kinetics

16. Chemical Equilibrium

17. Acid and Base Equilibrium

19. Chemical Thermodynamics

20. Electrochemistry

21. Nuclear Chemistry

22. Organic Chemistry

23. Chemistry of the Nonmetals

24. Transition Metals and Coordination Compounds

[BOOK CHEM] Clutch Version

Weak Acid Strong Base Titrations

Whenever a WEAK ACID reacts with a STRONG BASE we use an ICF Chart to determine the pH of the solution.&#160;

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

Titrations of Diprotic and Polyprotic Acids

A diprotic or polyprotic buffer can be approached in a way similar to monoprotic buffers. The key difference is that multiple pKa values will be involved.&#160;

Buffer

Weak Base Strong Acid Titrations

Whenever a&nbsp;WEAK BASE reacts with a&nbsp;STRONG ACID we use an&nbsp;ICF Chart to determine the pH of the solution.&nbsp;