A solution (total volume =53.491 g/mol). Kb = 1.8 · 10-5. Calculate:1L) of 0.4 M NH3 contains 12.78 g of NH4CI (MW =(a) The observed variation in pH upon bubbling of 0.05 moles of HCI gas inthis solution.

First we would Calculate initial pH of solution before adding HCl. Then pH after adding HCl is…

A solution (total volume = 1L) of 0.4 M NH3 contains 12.78 g of NH4CI (MW = 53.491 g/mol). Kb = 1.8 · 10-5. Calculate: (a) The observed variation in pH upon bubbling of 0.05 moles of HCI gas in this solution.

A solution (total volume = 1L) of 0.4 M NH3 contains 12.78 g of NH4CI (MW = 53.491 g/mol). Kb = 1.8 · 10-5. Calculate: (a) The observed variation in pH upon bubbling of 0.05 moles of HCI gas in this solution.

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: Calculate the pH of a solution (aq., 25 oC) prepared by dissolving 48.026 g of ammonium nitrate (mm…

A: In this question, we want to determine the pH of a solution. You can see details Solution below…

Q: 18) How many grams of sodium fluoride (MM =41.988 g/mol) must be added to 250.0 mL of a 0.100 M…

A: This question based on formula of acidic buffer NaF and HF is acidic buffer The answer is c that…

Q: Calculate the equilibrium pH of a solution that is initially 0.1M in both HCH COO and NaCH COO. Ka…

A: The objective of the question is to calculate the equilibrium pH of a solution that is initially…

Q: Q1a): Arrange the following 0.10 M aqueous solutions in order of increasing PH: Caso,, H,SO, NH,NO,…

A: (1a) The different types of salts formed by Acids and bases , if during the formation of salt,…

Q: A solution is prepared at 25 °C that is initially 0.45M in methylamine (CH,NH,), a weak base with…

A: Solution- Here we have basic buffer with Kb ; basic ; CH3NH2=0.45 M Acid; CH3NH3Br = 0.49M Kb= 4.4…

Q: A solution is prepared at 25 °C that is initially 0.22M in trimethylamine ((CH3)₂N), a weak base…

A: Buffer solution: The solution that resists the change in pH is known as a buffer solution. The…

Q: Calculate the pH of a solution obtained by mixing 154.52 mL of 0.28 M CH3COOH with 154.52 mL of 0.28…

A: Note: As per the guidelines, solution of 1st question has been made. For the expert solution of 2nd…

Q: How many grams of NH4Cl (53.49 g/mol) must be dissolved in 0.639 L of solution in order to obtain a…

A: we need to find mass of NH4Cl in the solution for a pH 4.79

Q: Calculate the pH of a solution that is 1.314 M HF, 0.442 M NaOH, and 0.719 M NaF. For HF K = 7.2 x…

A: Here we have NaOH which is a strong base and will completly dissociate on reacting with HF.

Q: Do not give handwriting solution.

Q: NH3 is a weak base (K₁ = 1.8 x 10-5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

A: A solution is given that is 0.036 M in NH4Cl at 25oCKb = 1.8*10-5Need to find the pH

Q: A 0.100 L solution is composed of 0.500 M (CH3)2NH and 0.500 M (CH3)2NH2Cl at 25 oC. What is the pH…

A: The objective of the question is to calculate the pH of the solution after the addition of .A buffer…

Q: HCN is a weak acid (K₁ = 6.20 x 10-10), so the salt, KCN, acts as a weak base. What is the pH of a…

Q: Tryptamine (C10H12 N2) is a stimulant found in chocolate. Its molecular structure is shown below.…

A: Buffer solution is a type of solution that resists the change in its pH on adding small quantity of…

Q: Calculate the pH of a solution obtained by mixing 25.00 mL of 0.20 M NH3 with 25.00 mL of 5.0 x 10-2…

Q: 6.5 g of sodium acetate was dissolved in 100 mL of water to give a final volume of 106 mL. If the Ka…

A: Sodium acetate dissociates in water into sodium and acetate ions. Sodium ions react very little with…

Q: A solution (total volume = 1L) of 0.4 M NH3 contains 12.78 g of NHẠCI (MW = 53.491 g/mol). Kb = 1.8…

Q: Write the chemical reactions whose equilibrium constants are K, and K, for imidazole (C, H, N,) and…

Q: 2.) A 3.90 g sample of aniline (C.H$NH2, K» = 4.3 x 100 at 25°C) is dissolved in sufficient water to…

A: ·Mass of Aniline = 3.90 g·Volume of solution = 100 mLAs we know that,·Molar mass of aniline = 93…

Q: The propionate lon, CH CH,COO", reacts with water as a weak base: CH CH,COO", (aq) + HO)…

Q: A solution of HF was made up at 0.050 M in water and the HF Ka = 7.2 x 10-4 at 25° C. (a) Write a…

A: Given, [HF] = 0.050 M Ka = 7.2 x 10-4 , T = 25 oC = 298 K

Q: mass of NaCH3COO must be dissolved in 400 mL of 0.46 M CH3COOH in order to prepare a solution with…

Q: Calculate the pH of a 0.234 M solution of NaNO₂. The ionization constant, K,, for the acid, HNO₂, is…

A: In this question we need to find pH of 0.234 M NaNO2 solution Given that, Ka for HNO2 = 4.60×10-4

Q: Consider the reaction of 75.0 mL of 0.350 M C₅H₅N (Kb = 1.7 x 10⁻⁹) with 100.0 mL of 0.393 M HCl.…

Q: ||| O ACIDS AND BASES Predicting the qualitative acid-base properties of salts Consider the…

A: The question is based on the concept of salt hydrolysis. we need to arrange the salts in increasing…

Q: A solution is prepared at 25 °C that is initially 0.46M in methylamine (CH,NH,), a weak base with…

A: Kb = 4.4 * 10-4pKb = -logKbpKb = -log(4.4 * 10-4)pKb =3.36

Q: A sample of 7.80 L of NH3 (ammonia) gas at 22 ∘C and 735 torr is bubbled into a 0.400 L solution of…

A: To calculate the pH of the resulting solution after adding ammonia () gas to hydrochloric acid (HCl)…

Q: pH

Q: If someone takes a breath and the lungs expand from 4.5 L to 5.8 L in volume, and the initial…

Q: HCN is a weak acid (Ka = 6.20 x 10-10), so the salt, KCN, acts as a weak base. What is the pH of a…

A: Given: Ka of HCN = 6.20×10-10 KCN = 0.0675 M we have to determine the pH ? Kb = Kw / Ka = 1 ×…

Q: A solution of carbonate (pKa = 6.3, 10.3) contains 0.0100 mol HCO3- and 0.00500 mol CO32-. Calculate…

A: Given : pka1 = 6.3 pKa2 = 10.3 [ HCO3- ] = 0.0100 [CO32-] = 0.00500 To calculate : pH

Q: prepared by mixing 25.0 g HC2H3O2 and 25.0 g NaC2H3O2 in 800.0 mL solution (Ka HC2H3O2 = 1.8 x 10-5)

Q: What mass (in g) of potassium fluoride should be added to 0.50 Lof 0.255-M HF(aq) at 25 °C to give a…

A: Given: Concentration of HF = 0.255 M Volume of solution = 0.50 L pH of buffer solution = 3.85 And…

Q: this question. Calculate the pH of a solution that is prepared by dissolving 0.168 mol of…

A: The two given acids dissociate partially as- C6F5COOH→C6F5COO- + H+ Ka= 3.30×10-2HClO →H+ +…

Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

A solution (total volume =
53.491 g/mol). Kb = 1.8 · 10-5. Calculate:
1L) of 0.4 M NH3 contains 12.78 g of NH4CI (MW =
(a) The observed variation in pH upon bubbling of 0.05 moles of HCI gas in
this solution.

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

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 2 images

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

Calculate the pH of a solution prepared by dissolving 0.350 mol of benzoic acid (C7H502H) and 0.200 mol of sodium benzoate (NaC7H502) in water sufficient to yield 1.00 L of solution. The Ka of benzoic acid is 6.50 x10^-5.
A solution is prepared at 25 °C that is initially 0.48 M in diethylamine ((C,H5)¸NH), a weak base with K,=1.3 × 10 -3 and 0.024M in diethylammonium bromide ((C,H5) NH,Br). Calculate the pH of the solution. Round your answer to 2 decimal places. pH olo Ar
What is the pH of a solution that is 0.21 M CH3NH2 (methylamine) and 0.31 M CH3NH3Cl (methylammonium chloride)? (Assume Kw is 1.0 ✕ 10−14.)
Give detailed Solution
A solution is prepared at 25 °C that is initially 0.29M in chloroacetic acid (HCH,CICO,), a weak acid with K,=1.3 × 10 and 0.34M in sodium chloroacetate (NaCH,CICO,). Calculate the pH of the solution. Round your answer to 2 decimal places. pH = 0 ?
Calculate the pH of a solution containing 0.70 M HC2H3O2 and 0.25 M NaC2H302. The K, for HC,H;0, is 1.8x10-5. pH =
The substance acetylsalicylic acid (aspirin) (HC,H704) is a weak acid (Ka = 3.0×10-4). What is the pH of a 0.191 M aqueous solution of potassium acetylsalicylate, KC,H704? pH = || This solution is
The pH of which of the following solutions will decrease by 1.00 pH unit when diluted with water to 10 times its original volume? 0.10 M HCI 0.10 M NAOH 0.10 M CH3COOH 0.10 MCH3COO Na" A mixture of 010 M CH;COOH and 0.10 M CH3COO'Na*
Please give calculation with explanation.
A solution is prepared at 25 °C that Is initlally 0.43M in dimethylamine ((CH, NH, a weak base with K, =5.4x10, and 0.15M in dimethylammonlum -4 and 0.15M In dimethylammonium bromide ((CH,),NH,Br) ((CH,) NH,Br). Calculate the pH of the solution. Round your answer to 2 decimal places. bгomide 2. pH Explanation Check 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privac hp
The ion HTe− is an amphiprotic species; it can act as either an acid or a base.(a) What is Ka for the acid reaction of HTe− with H2O?(b) What is Kb for the reaction in which HTe− functions as a base in water?(c) Demonstrate whether or not the second ionization of H2Te can be neglected in the calculation of [HTe−] in a 0.10 M solution of H2Te.
Original concentration of Acetic Acid was 0.1033 M and NaOH was 0.1104 M there is part a done, need to do part B