Answered: What is the pH of a 0.100M NH3…

What is the pH of a 0.100M NH3 solution? Kb for NH3 is 1.8 x 10-5? NH3(aq) + H2O() = NH4+(aq) + OH-(aq). a. 1.87 b. 2.87 C. 11.13 O d. 12.13

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: The pH of a solution made up to contain 0.240 M H3PO4 and 0.480 M NaH2PO4 is- (Ka1= 7.11 x 10-3;…

A: Buffer solution are which can resist any change in PH when either acid or base are added and the PH…

Q: What is the concentration (in M) of H + ions in a solution at 25.0 °C with pH = 4.146? a. 9.85…

A: Given: pH = 4.146 The pH of a solution is given by : pH =-log [H+]

Q: . Which of the following solutions the has the lowest pH? A. 0.50 M HNO₂ (Ka = 4.6 x 10-4) B. 5.00 M…

A: Answer:- This question is answered by using the simple concept of calculation of pH of weak acids…

Q: 11. The pH of a Ba(OH)2 solution is 10.00. What is the Ht ion concentration of this solution? A. 4.0…

A: pH is used to determine the concentration of hydronium ion.

Q: The pKa for HCN(aq) is 9.21. What is the pH of a 1.245 M solution of NaCN? O a. 11.25 O b. 1.24 O c.…

A: this is the salt of weak acid and strong base. so ,we will use hydrolysis equation of weak acid and…

Q: 4. Which solution has the lower pH? a. 0.1M HCl or 0.1M HC2H30₂ b. C. 0.1M NaOH or 0.1M NH3(aq) 0.1M…

A: We have find out the answer.

Q: 3. In the reaction below, H2O is a(n): H2SO; +H2O → H;O*+ HSO; a. Base b. acid Su conjugate acid d.…

A: “Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: A solution is made by dissolving 0.0015 mole Ba(OH)2 in enough water to make 1.50 liter of solution.…

A: dExplanation:

Q: A sample of water from the Chesapeake Bay has [H3O+] = 3.1 x 10-6 M. Which statement below…

Q: What is the pH of a solution that is 0.150 M NH3 and 0.200 M NH4CI? Kb of NH3 = 1.8 x 10-5 O9.26…

Q: Calculate the pH of a 0.30 M solution of NH 4Cl (Kb for NH 3 = 1.8 x 10 -5). a. 11.67 b.…

A: NH4Cl is the salt weak base NH4OH and a strong acid HCl therefore hydrolysis constant Kh will be…

Q: Find the conjugate acid - base pairs for the following reactions. a. Co + H,0 = HCO, + OH b. HF +…

Q: What is the pH of a 3.3 × 10-4 M CSOH solution?

Q: What is the pH of a solution containing a mixture of 0.50 M HCN and 0.040 M NaCN? (Ka = 4.9 x 1010…

A: Answer :- HCN is a weak acid and NaCN is its conjugate Salt . This solution is basically acts as a…

Q: This compound is a weak organic base: C18H21O3N + H2O C18H21O3NH+ + OH-…

Q: What is the pH of a 0.010 M solution of aqueous Sr(OH)2? a. 10.2 b. 2.0 c. 9.0 d.…

A: To determine the pH of a basic solution, the pOH is determined first and then pH is calculated using…

Q: 37. A solution has a pH of 10.65. What is the [H3O+] value for this solution?\ a. 2.2 x 10-11 b. 4.5…

A: In Chemistry, pH is a scale which is used to specify the acidity or basicity of an aqueous solution.…

Q: a. What is the hydroxyl concentration of the ammonia solution? b. What is the pOH of the ammonia…

A: Given: Volume of ammonia solution= 300ml Concentration of ammonia solution= 0.05M The density of the…

Q: 6. Which solution has the highest pH? A. 0.10 M HCIO4 (aq) B. 0.10 M HBrO4 (aq) C. 0.10 MHCI0(aq) D.…

A: pH is defined as negative logarithm of hydrogen ions

Q: Calculate the concentration of OH- in a solution that contains 6.5 x 104 M H30 + at 25°C. Identify…

A: A solution is acidic if pH<7 Basic if pH>7 pH = -log[H+] pOH = -log[OH-] pH+pOH = 14

Q: pH pOH [H*] [OH]] Acidic, Basic or Neutral? a. Solution 9.60 a M M pH РОН [H*] [_HO] or Neutral?…

Q: 4. Calculate the pH of each of the following solutions of strong acids and bases: a. 0.0010 M HCI b.…

Q: From what acid and what base are these salts below made from? a. Ca(NO3)2 b. NH4Br c. BaCl2

Q: What is the pH of the solution when 50.0 mL of 0.10 M KOH and 50.0 mL of 0.12 M HCl are mixed?…

A: Given HCl + KOH -> KCl + H2O 0.12M 0.10M 50ml 50ml pH =…

Q: Calculate the pH of a solution that's 0.65M in NaF and 0.75M in HF. (HF. Ka = 7.2 x 10-4)? A.3.08…

Q: What is the pH of a solution made of 0.15M NH3 and 0.23M NH4Cl? where the Kb= 1.8 x 10-5. A. 4.61…

Q: Which of the solutions listed below has the lowest pH? A. Pure H20 B. 2.5 x 10° M HNO3 C. 0.10 M…

A: Given the solution have lowest PH from following solution a) pure H2O b) 2.5 * 10^-5M HNO3…

Q: 6. What is the pH of 0.025 M (CH3)3N(aq)? For (CH3)3N, K, 6.5 × 10-5, 9.81 11.11 12.40 11.91 - | |…

A: (CH3)3 is weak base hence it dissociated feabily in aqueous solution

Q: The pH of a 4.6 x 10 -4 M Ca(OH) 2 solution at 25 °C is _____. Note that Ca(OH) 2 is a strong base.…

A: Given: The concentration of the Ca(OH)2 solution = 4.6 x 10 -4 M We have to calculate the pH of the…

Q: Arrange the following solution from lowest pH to highest pH:

A: Acid and base are the chemical compounds which upon adding in water change the pH value accordingly.…

Q: Calculate the pH of a 0.12 M solution of NaC2H3O2 (for HC2H3O2 Ka= 1.8 x 10 ^-5). A. 5.09 B. 8.91…

A: Answer:When salt of weak acid and strong base is added in water it gets hydrolyzed to produce OH-…

Q: Calculate the H3O+ and pH of each polyprotic acid solution. a. 0.350 M H3PO4 b. 0.350 M H2C2O4

Q: None

A: Step 1: Calculation of the H+ concentration Given, pH = 6 We know, => [H+] = 10-pH => [H+] =…

Q: The concentration of H+ ions in a solution is 0.315 M. a. Calculate the concentration of OH– ions…

A: Applying formula PH= -log[H+]

Q: The pk, for HCN(aq) is 9.21. What is the pH of a 1.245 M solution of NaCN? O a. 11.95 O b. 1.24 O c.…

Q: 20. What is the pH of a solution with [H3O*] of 5.8 x 105 a. 5.80 b. 4.24 C. 9.76 d. 10.60 e. 5.00

A: pH of a solution measures the acidity of that solution. pH from the solution can be determined from…

Q: 13. What is the pH of a 0.0 1 5M Ca(OH)2 solution? a. 1.52 b. 12.18 c. 12.48 d. 1.82

A: The required equation is given below.

Q: What is the concentration of H* ions in HCI whose pH is 8.3?

A: pH of the solution is equal to the negative logarithm of H+ ion concentration. Write the expression…

Q: a. A solution of HNO3 has a pH of 3.69. What is the molarity of the solution? Molarity |M b. A…

A: We know that, HNO3 is strong acid. So, it is completely dissociated. Thus, pH= -log[H+] Thus, [H+]…

Q: ample human blood was measured to pe 7.52 at 25°C. Calculate pOH, CH+], and [OH-] for the sample.…

A: pH +pOH = 14 pH = -log[H+] pOH = -log[OH-]

Q: 40. The pH of a sample of human blood was measured t be 7.52 at 25°C. Calculate pOH [H+], and [OH-]…

Q: Without using a calculator, determine the pH and pOH of each solution. Rank the solutions from most…

A: pH of the solution is equal to the negative logarithm of hydronium ion concentration while pOH is…

Q: 1. Calculate the pH of the following: a. A solution whose pOH = 8.95 b. 6.37 M HCI c. 5.25 M Ca(OH)2…

A: pH : it can define as the negative logarithm of H+ ion concentration. When pH > 7 solution is…

Q: Which of the solutions listed below has the lowest pH? A. Pure H2O B. 2.5 x 10-5 M HNO3 C.…

A: Lowest pH mean stronger acid and higher pH mean stronger base .

Q: C. A 0.0543 M solution of a weak acid HA has a pH of 4.87. Calculate K, and % ionization of a the…

A: There is more than one question, and all are different. As per answering guidelines I can answer…

Q: What is the pH of a solution that is 0.40 M in HCN? The Ka for HCN is 4.0x10-10. a. 0.40 b. 9.40 c.…

Q: 3. In the reaction below, H;O is a(n): H;SO, + H:O → H;O*+HSO; a. Base 4. What is the pH of a 1.53 x…

A: The question is based upon acid base concept and we know that acid are those molecule which donate…

Question

What is the pH of a 0.100M NH3 solution? Kb for NH3 is 1.8 x 10-5?
NH3(aq) + H2O() = NH4+(aq) + OH-(aq).
a. 1.87
b. 2.87
C. 11.13
O d. 12.13

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps with 3 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

-117. Determine [OH¯], [H*], and the pH of each of the following solutions. a. 1.0 M KCl b. 1.0 M KC₂H3O₂
1. A 0.01 M aqueous solution of __________ will have a pH of 7.0 (neutral) at 25.0°C. a. NaOCl b. NH4Cl c. Ca(C2H3O2)2 d. KCl
The pH of a solution is 3.38. What is the OH concentration in the solution? esc 24 % 4. 6. 7 E R. T U lab S F Go CODs lock
What is the pH of a solution with [OH¯] = 1 x 10-5M ? A. 1 x 10-9 %3D B.9 C.5 D.5 E. 9
3. Calculate the pH of the following aqueous solutions. a. 2.62 x 10-1 M HCl b. 9.6 x 10-12 M HNO3 c. 5.00 mL’s of solution a. diluted to 100.0 mL in a volumetric flask.
17. Find the pH of 0.3500 M HNO₂(ag) solution @ 25 °C. K, for HNO₂ = 4.6 x 10-4 HNO₂ + H₂O NO₂ + H₂O+ A. 4.79 B. 3.79 C. 6.55 D. 8.72 18. What is the percent ionization of a 3.34 M solution of nicotinic acid, HC6H4NO₂? (K₂ = 1.4 x 10-5 @ 25 °C) HC6H4NO₂ + H₂O C6H4NO₂ + H₂O+ A. 4.68% B. 6.84 % C. 0.2% D. 48.8%
1. The equilibrium constant, K, for a monoprotic acid (propionic acid) is 1.3 x 10-5. Which of the following is the correct value of K, for the propionate ion, the conjugate base of propionic acid? a. 1.3 × 10⁹ b. 1.3 × 10-19 c. 7.7 x 104 d. 1.3 × 10-5 e. 7.7 x 10-10 -. Which of the following expressions correctly describes the equilibrium constant K, for the reaction given below? 4 NH3(g) +5 O₂(g) 4 NO(g) + 6 H₂O(g) a. Kc = b. Kc = c. Ke= d. Ke= e. Kc = [NO₂][H₂O] [NH3][0₂] 4[NH3]+5[0₂] 4[NO]+6[H₂0] [NO][H₂O16 [NH,[0₂] [NH₂] [0₂] [NO][H₂O] 4[NO]+6[H₂0] 4[NH3]+5[0₂]
Acetic acid (HC2H3O2) is a weak aicd ( Ka= 1.8 x 10^-5). Calculate the pH pf a 12.1 M HC2H3O2 solution. A. -1.08 B. 3.66 C. 1.83 D. 1.08 E. 12.17
If the following salts are each dissolved in water to form 0.1 M solutions at 25 °C, which will have a pH of 7.0? I. NaOCl II. KCl III. NH4Cl IV. Ca(CH3COO)2 Select one: a. II and III b. I and IV c. III and IV d. II only
5. Find the pH of each mixture of acids. a. 0.115 M in HBr and 0.125 M in HCOOH b. 0.185 M in HCOOH and 0.225 M in CH3COOH austdo of noi fo 6. Arrange the solutions in order of increasing acidity. a. NaCl, NH4Cl, NaHCO3, NH4CIO2, NaOH b. Which is a stronger base, S²- or Se²- ?
A 1.0-liter solution contains 0.25 M HF and 0.41 M NaF (Ka for HF is 7.2 x 10-4). What is the pH of this solution? O a. 3.36 O b. 10.64 O c. 2.93 O d. 3.14 O e. 0.21
Calculate the pH of a solution containing 0.010 M HCOOH (Ka = 1.90 × 10-4) and 0.061 M HCI. A. 0.39 B. 0.92 C. 0.68 D. 1.21 E. 1.92