21) What will be the pH (aq., 25 °C) of 100.0 mL of asolution of 1.00 M C̟H̟NH,Br and 1.50 M C,H¸NH,after2.00 mL of 10.00 M HC1 has been added to it?К. СН.NH,3D 5.60 х 10*b) 10.8e) 9.24c) 8.84f) 10.6а) 3.65d)9.82

Firstly Calculate the mmoles of salt, weak base and acid : salt : C2H5NH3+ , weak base : C2H5NH2…

21) What will be the pH (aq., 25 °C) of 100.0 mL of a solution of 1.00 M C̟H̟NH̟B and 1.50 M C,H,NH, after 2.00 mL of 10.00 M HC1 has been added to it? К. СHNH,3D 5.60 х 10* а) 3.65 9.82 b) 10.8 e) 9.24 c) 8.84 f) 10.6 d)

21) What will be the pH (aq., 25 °C) of 100.0 mL of a solution of 1.00 M C̟H̟NH̟B and 1.50 M C,H,NH, after 2.00 mL of 10.00 M HC1 has been added to it? К. СHNH,3D 5.60 х 10* а) 3.65 9.82 b) 10.8 e) 9.24 c) 8.84 f) 10.6 d)

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: What is the pH of an aqueous solution that consist 40.0 mL of 0.050 M HI and 30.0 mL solution…

A: Mixture of strong and weak acid will release proton. The strong acid will release according to its…

Q: Calculate the pH when 45.0 mL of 0.200 M HBr is mixed with 46.0 mL of 0.400 M CH NH2 (Kb = 4.4 ×…

A: Given: Concentration of HBr = 0.200 MVolume of HBr solution = 45.0 mL = 0.045 L…

Q: You have 50.0mL of 0.522M NH3. Kb = 1.8x10-5 You add 15.0mL of a 0.05M HCl solution. What is the pH…

A: The objective of this question is to calculate the pH of a solution after the addition of a certain…

Q: 19) Calculate the pH of a solution (aq., 25 °C) prepared by dissolving 48.026 g of ammonium nitrate…

A: Given: Mass of NH4NO3=48.026g Molar mass of NH4NO3=80.043 g/mol Volume =2.00L…

Q: Sodium nitride (NaNO2) is often used as a preservative for meats. a) Knowing that the Ka of nitrous…

A: Salt hydrolysis mainly takes place when one of the component of salt is weak. The weak part of a…

Q: What is the pH of a 100.0 mL 0.0500m HCN(aq) solution which is mixed with 5.00 mL 0.200 M KOH(aq) ?…

Q: What is the pH of a solution comprised of 0.75 M formic acid (HCHO2) and 0.63 M formate (CHO2-)?

A: Given information: Concentration of formic acid = 0.75 M Concentration of formate = 0.63 M

Q: In a liter of 0.2F solution of propionic acid, HCSHO2_it has ionization constant of 1.34 x 10,…

Q: You have 50.0mL of 0.520M NH3. Kb = 1.8x10-5 You add 15.0mL of a 0.05M HCl solution. What is the pH…

A: The objective of this question is to calculate the pH of a solution after the addition of a certain…

Q: Calculate the pH of the solution obtained by mixing 25.00 mL of 0.0745M HX and 25.00 mL of 0.0535M…

Q: mL CSOH added 5.00 10.00 15.00 20.00 25.00 OA HW pKa = 7.46 O B. HD pKa = 5.89 OCHG pKa = 6.85 ÖD.…

A: Molarity of Acid = 0.350 M Volume of Acid = 20 mL Mmol of Acid = M × V = 0.350 × 20 = 7.0 mmol…

Q: (1) HNO, H,SO, (2) Fe, HCI; HO CI (3) ACCI, (CH;CH2)N (4). SnBu, Pd(Ph,P). base

A: The above compound undergoes a sequence of reactions to give the final compound. It is a multistep…

Q: Calculate the pH of the solution obtained by mixing 25.00 mL of 0.0745M HX and 25.00 mL of 0.0535M…

Q: Calculate the pH of a mixture containing 0.266 mol HBz and 0.124 mol NaBz dissolved to 500.0 mL with…

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

Q: e pH

Q: Calculate the pH after addition of 22.55 mL of 0.1298 M HBr to 25.00 mL of 0.1529 M CH 3NH 2. K b(CH…

Q: Which of the following species cannot act as a Lewis base? A) NH- B) CH4 C) NH3 D) H2S E) S2-…

Q: 8-The following titration curve is the kind of curve expected for the titration of a base (a)…

A: The titration curve is a plot between pH (dependent variable) and the volume of titrant added…

Q: A chemist must prepare 800.0 mL of nitric acid solution with a pH of 1.00 at 25 °C. He will do this…

A: The volume of the diluted solution of nitric acid is .The pH of the diluted solution of nitric acid…

Q: What is the pH of a solution after 0.00200 mol of HNO3(aq) (100. mL) has been combined with 0.00100…

A: We have to calculate the pH of solution.

Q: A buffer solution could be made by mixing equal amounts of citric acid and a solution containing.…

A: Given a citric acid buffer solution. Fill the correct option.

Q: Consider equimolar solutions of each of the following compounds; rank them in order of increasing…

A: -> pH = -log[H+] -> As acidity increases H+ concentration increases and pH decreases. ->…

Q: Write the acid or base dissociation equation for Sr(OH)2 b.) Calculate the pH of a solution…

A: As an aqueous solution of strontium hydroxide dissociates completely in water because it is strong…

Q: a) 25.0 ml of 0.80M KCI + 35.0 ml of 0.40M KOH b) 20.0 ml of .20M HCI + 30.0 ml of 0.10M NaOH c)…

Q: o) 10 ml, 0-M HCL is udded to j00 ml of asal.tron which is 0.1M both in HOAC and Na OAC. 8y how many…

Q: You have 50.0mL of 0.514M NH3. Kb = 1.8x10-5 You add 15.0mL of a 0.05M HCl solution. What is the pH…

A: The pH of the final solution after adding HCl is approximately 5.13.Explanation:First, let's…

Q: . If BaCl2 completely dissolves in water, what is the ionic strength of a 0.0300 F solution of…

Q: 1. Consider a 0.0020 M (CH3)3N aqueous solution. (a)Write a mass balance (there is only one) and…

A: Answer: Trimethyl amine is a weak base, on adding in water it will furnish OH- ions and will form a…

Q: Step by step please

A: The pH of the salt is calculated by using the equation,

Q: What is the percent dissociation of a 0.1250M benzoic acid solution if its pH=2.59?

Q: 3. Calculate the pH of a mixture of 30.00 mL of 0.4508 M HBr and 18.00 mL of 0.1162 M Ca(OH)2.…

A: Given,Molarity of HBr = 0.4508 MVolume of HBr = 30.00 mLMolarity of Ca(OH)2 = 0.1162 MVolume of…

Q: Calculate the pH for each of the following cases in the itiration of 25.0 mL off 0.200 M NH3 (aq)…

Q: You have 50.0mL of 0.541M NH3. Kb = 1.8x10-5 You add 15.0mL of a 0.05M HCl solution. What is the pH…

A: The objective of this question is to calculate the pH of a solution after the addition of a certain…

Q: 1. The pH of 100.0 mL of 0.100 M N(CH₂), was 11.37. Calculate pK, for N(CH₂), and pK, for HN(CH₂).

A: The question is based on the concept of chemical equilibrium. we need to calculate pka value for…

Q: You have 50.0mL of 0.527M NH3. Kb = 1.8x10-5 You add 15.0mL of a 0.05M HCl solution. What is the pH…

A: The objective of this question is to calculate the pH of a solution after the addition of a certain…

Q: Calculate the pH if 68mL of 0.150M ethylamine (pKb=3.252) is added to 68 mL of 0.128 M KOH. Assume…

A: Ethylamine is a weak base with pKb of 3.252. KOH is strong base. There is no reaction between strong…

Q: What volume of 0.0100 M NaOH must be added to 1.00 L of 0.0500 M HOC1 to achieve a pH of 8.00? (K of…

A: Let volume of NaOH be X L Molarity of NaOH = 0.01 M Molarity of HOCl = 0.05 M Moles = Molarity ×…

Q: Explain the attachment

A: Given : Concentration of NaCH3COO = 0.20 M Concentration of HCl = 0.200 M Volume of NaCH3COO…

Q: 1 out of Calculate the pH of a 0.40M solution of sodium acetate (NaCH,COO) given that the K, of…

A: NaCH3COO solution means salt hydrolysis. NaCH3COO is made up of weak acid acetic acid and strong…

Q: The pH of an aqueous solution of 0.237 M ammonium chloride, NH4Cl(aq), is (Assume that Kb (NH3) =…

A: We have to calculate the pH of ammonium chloride solution

Q: 17. Find the pH of a solution that is prepared by combining 0.0034M lactic acid, CH;CH(OH)COOH, and…

A: The pH of the solution prepared by combining Lactic Acid and Sodium Lactate is given as -

Q: 14. What is the pH of a 2.58 M solution of ZnCl(aq)? (K,-1.0 x 10 for Zn(H₂O),"") 5.59 11.71 4.29 d.…

A: Concentration of ZnCl2 (aq) = 2.58 MKa = 1 x 10-9 We have to calculate the ph of the resulting…

Q: If 50.00 ml of 1.00M HC,H,O; (K, = 1.8 x 10*) is titrated with 1.00 M NaOH. What is the pH of the…

A: Volume of CH3COOH = 50ml Concentration of CH3COOH = 1M Concentration of NaOH = 1M Ka = 1.8×10-5 We…

Q: Ascorbic acid C5H7O4CO2H (Ka =7.9x10^-5) also known as vitamin C is an essential nutrient for all…

Q: Calculate the pH of solution made by combining 100 ml of 0.28 М НС,Н;0; and 50 ml of 0.36 M NaOH, Ka…

Question

21) What will be the pH (aq., 25 °C) of 100.0 mL of a
solution of 1.00 M C̟H̟NH,Br and 1.50 M C,H¸NH,
after
2.00 mL of 10.00 M HC1 has been added to it?
К. СН.NH,3D 5.60 х 10*
b) 10.8
e) 9.24
c) 8.84
f) 10.6
а) 3.65
d)
9.82

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Step 5

Step by step

Solved in 5 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

You have 50.0mL of 0.520M NH3. Kb = 1.8x10-5 You add 15.0mL of a 0.05M HCl solution. What is the pH of this solution?
You have 50.0mL of 0.520M NH3. Kb = 1.8x10-5 You add 15.0mL of a 0.05M HCl solution. What is the pH of this solution?
What is the pH of the resulting liquid: 13.0 mL 61.0 mM HNO3 and 12.0 mL 39.0 mM HBr?Please show complete solution, thank you.
Help. Please order these esters from most stable to least stable C=O.
Calculate the pH when 30.0 mL of 0.200 M HBr is mixed with 30.0 mL of 0.400 M CHNH: (Kb = 4.4 x 10*).
A solution is known to contain 0.843 moles of a C5H5N and 0.674 moles of C5H5NH+. The Kb of C5H5N is 1.70 * 10-9. What is the pH of this solution.
19. Consider the weak acid phenol (C6H5OH), for which Ka = 1.05 ×10-10 in aqueous solutions at 25°C. What is the pH of a 0.850 M aqueous phenol solution at 25°C? A) 4.02 B) 5.02 C) 8.95 D) 9.98 E) none of these
What is the pH of a solution prepared by diluting 195.7 mL of 1.55 M HNO3 (Ka>>1) to a total volume of 8.98L? Please report your answer to 3 sig figs.
10. 0.02 mole of NH,OH and 0.03 mole of NH,Cl are mixed in 300 ml, what is the pH of the solution? Kb = 1.8 X 10s
The pH for 6.1 × 10-4 M solution of cocaine, a weak base, is 9.60. Determine the value of Kb for cocaine. 1 2 NEXT Let cocaine be represented by the generic base, B. Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. B(aq) H20(1I) OH (aq) BH*(aq) + + Initial (M) Change (M) Equilibrium (M) 5 RESET 6.1 x 10-4 9.60 -9.60 2.5 x 10-10 -2.5 x 1010 4.0 x 10-5 -4.0 x 10-5 2.1 x 10-4 -2.1 x 10-4 5.7 x 10-4 -5.7 x 10-4 +x x + 2.5 x 1010 -x x - 2.5 x 1010 x + 4.0 x 10-5 x - 4. 10-5
3b.) The Ka of acetic acid is 1.8 x 105. Calculate the pH of the following solutions: b. A solution consisting of 0.10 M acetic acid (HC2H302) and 0.50 M sodium acetate (NAC2H3O2).
The two molecular scenes below depict the relative concen-trations of H₃O⁺ (purple) in solutions of the same volume (withcounter ions and solvent molecules omitted for clarity). If the pHin scene A is 4.8, what is the pH in scene