Log in
Chemistry
1
answer
0
watching
849
views
12 Dec 2019

A lab technician adds 0.015 mol of KOH to 1.00 L of 0.001 M Ca(NO3)2. Ksp= 6.5x10^-6 for Ca(OH)2. Which of the following statements is correct?

- Calcium Hydroxide precipitates until solution is saturated.

- the solution is unsaturated and no precipitate forms

- the concentration of calcum ions is reduced by the addition of the hydroxide ions.

- one must know Ksp for calcium nitrate to make meaningful predictions.

- The presence of KOH will raise the solubility of Ca(NO3)2

Watch
1
answer
0
watching
849
views

For unlimited access to Homework Help, a Homework+ subscription is required.

Elin Hessel
Elin HesselLv2
13 Dec 2019

Unlock all answers

Get 1 free homework help answer.
Already have an account? Log in
Share
discord banner image
Join us on Discord
Chemistry Study Group
Join now

Related textbook solutions

Basic Chemistry
5 Edition,
Timberlake
ISBN: 9780134138046
Principles of Chemistry Molecular Approach
4th Edition,
Tro
ISBN: 9780134112831
Chemistry: Structure and Properties
2nd Edition,
Tro
ISBN: 9780134293936
Principles of Chemistry Molecular Approach
3rd Edition, 2014
Tro
ISBN: 9780321971944
Chemistry: A Molecular Approach
3rd Edition,
Tro
ISBN: 9780321809247
Chemistry: A Molecular Approach
5th Edition,
Tro
ISBN: 9780134874371
Principles of Chemistry: A Molecular Approach
4th Edition,
Tro
ISBN: 9780134895741
Chemistry: The Central Science
14th Edition, 2017
Brown
ISBN: 9780134414232

Related questions

I would really appreciate it if someone showed me how to solve each of these problems instead of just giving the answers. I bolded the correct answer. Thank you

1. How many milliliters of a 5.0 x 10^-2 stock solution would you need to add to a final volume of 10 liters to obtain a solution with a pH of 3.60?

a. 50 mL

b. 34 mL

c. 13 mL

2. A 0.25 M solution of a hypothetical weak acid, HX has a pH of 3.42. What is the Ka value for this acid?

a. 8.8 x 10^ -6

b. 1.6 x 10^ -7

c. 5.8 x 10^ -7

3. What is the pH of a 0.30 M solution of magnesium hypochlorite(Mg(ClO)2)? For HClO Ka= 3.0 x10^ -8

a. 9.06

b. 3.06

c. 10.65

4. The pH= 2.84 for a 0.35 M pyridine hydrochoride, C5H5NHCl, solution. Based on this information, determine the Kb value of pyridine (C5H5N)

a. 9.4 x10^-8

b. 1.7x 10^ -9

c. 5.3 x 10^ -7

5. If you wanted to prepare a buffer composed of hypochlorous acid (HClO0 and potassium hypochlorite (KClO), how may moles of KClO would be added to 2 liters of a 1.0 M HClO solution to get a buffer with a final pH of 7.70? For HClO, Ka= 3.0 x 10^-8

a. 3.0 mol KClO

b. 1.2 mol KClO

c. 2.2 mol KClO

6. The pH of a solution by mixing 300 mL of 0.050 M HClO4 and 40.0 mL of 0.10 M Ba(OH)2 is?

a. 1.69

b. 1.77

c. 1.85

7. A 150 mL sample of 0.20 M HF solution is titrated with a strong base. What is the pH after adding 40 mL of 0.80 M NaOH? For HF, Ka= 6.8 x 10^-4

a. 13.11

b. 12.02

c. 10.37

8. A solution of Pb(NO3)2 is mixed with a solution of NaCl. A precipitate forms and analysis of the supernatant reveals the following concentrations of ions.

[Pb^2+] = 0.0062 M [NO3-]= 0.25 M [Na+]= 0.40 M [Cl-]= 0.054 M

Based on these data, what is the Ksp value for PbCl2(s)?

a. 7.2 x 10^-6

b. 5.6 x 10^-8

c. 1.8 x10^ -5

9. At an elevated temperature, Ksp= 7.5x 10^ -5 for Ca(OH)2. What is the pH of a saturated solution of a calcium hydroxide?

a. 13.06

b. 9.51

c. 12.73

QUESTION 1

Equal molar amounts of nitric acid (a strong acid) and methylamine (a weak base) are combined in an aqueous solution.

The pH of the resulting solution is:

greater than 7

close to 7

less than 7

QUESTION 2

A 1.00 L aqueous solution contains 0.10 mol acetic acid and 0.10 mol sodium acetate. The initial pH is 4.74. Calculate the pH after the addition of 0.049 mol of OH-.

QUESTION 3

Using the Henderson-Hasselbalch equation, calculate the pH of a buffer solution that contains 0.96 M NH4Cl and 0.33 M NH3.

QUESTION 4

A 10.0 mL volume of 0.49 M HNO3 is combined with a 15.0 mL volume of 0.58 M NaOH. Calculate the pH.

QUESTION 5

A diprotic acid is being titrated with a strong base. A volume of 0.0500 L of 0.0750 M diprotic acid (H2A+) is combined with 0.0150 L of 0.250 M NaOH.

Ka1 for the diprotic acid is 3.6 x 10-3.

Ka2 for the diprotic acid is 4.7 x 10-7.

Calculate the pH of the solution.

QUESTION 6

A saturated solution of Ca3(PO4)2 has a concentration of Ca2+ = 5.65 x 10-7 M and a concentration of PO43- = 9.80 x 10-8 M. Calculate Ksp for Ca3(PO4)2.

Answer in exponential notation. Examples:

Scientific Notation Exponential Notation

1.00 x 10-10 1.00e-10

5.00 x 105 5.00e5

QUESTION 7

A solution is prepared by combining 0.125 L of 0.020 M Pb(NO3)2 and 0.125 L of 0.050 M PbBr2. Does a precipitate of PbBr2 form? Ksp of PbBr2= 6.6 x 10-6

Yes, a precipitate forms.

No, a precipitate does not form.

QUESTION 8

Calculate the molar solubility of MgF2 in 0.37 M NaF at 25°C. Ksp = 7.4 x 10-11.

Answer in exponential format.

QUESTION 9

Determine the concentration of Ag+ in a solution prepared by adding 0.10 mol AgNO3 to 1.0 L of 3.9 M NH3.

Ag+(aq) + NH3(aq) [left right double arrow] AgNH3+(aq) K1 = 2.1 x 103

AgNH3+(aq) + NH3(aq) [left right double arrow] Ag(NH3)2+(aq) K2 = 8.1 x 103

Ag+(aq) + 2 NH3(aq) [left right double arrow] Ag(NH3)2+(aq) Kf = 1.7 x 107

QUESTION 10

Determine the molar solubility of MgCO3 at 25°C in pure water.

Ksp = 6.8 x 10-6

Weekly leaderboard

Home
Homework Help 3,900,000
Chemistry 830,000
Start filling in the gaps now
Log in