Calculate the acetate ion concentration in a solution prepared by dissolving 6.20x10-3 mol of HCI(g) in 1.00 L of 1.20 M aqueous acetic acid (Ka = 1.80x10-5). mol/L Submit Answer Tries 0/5 Calculate the pH of the above solution.

Calculate the acetate ion concentration in a solution prepared by dissolving 6.20x10-3 mol of HCI(g) in 1.00 L of 1.20 M aqueous acetic acid (Ka = 1.80x10-5). mol/L Submit Answer Tries 0/5 Calculate the pH of the above solution.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter14: Principles Of Neutralization Titrations

Section: Chapter Questions

Problem 14.38QAP

See similar textbooks

Related questions

Q: What mass of ammonium chloride should you add to 2.65 L of a 0.150 mol L-1 NH3 to obtain a buffer…

Q: Dashboard 10 Chem101 b Answered: At a particular tempe x i app.101edu.co Question 2 of 16 Submit…

Q: a) 1.00L of a buffer is created to be 0.100M in HOAC and 0.100M in NaOAc. What is the pH of the…

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: calculate the pH after 10.0, 20.0, 30.0, and 40.0 mL of a 0.100 M NaOH have been added to 40.0 mL of…

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

Q: A 0.344-M aqueous solution of a weak acid has a pH of 3.39. Calculate Ka for the acid. Ka = Submit…

Q: The first equivalence point for 40.00 mL of 0.1000 M H3PO4 is reached when 21.38 mL of 0.1871 M NaOH…

A: The question is based on the concept of chemical equilibrium. We have been given pH at first…

Q: ion: find the acidity function when adding 5 ml of NaOH Calculate the pH value when titrated between…

Q: The pH of a solution prepared by mixing 45.0 mL of 0.183 M KOH and 25.0 mL of 0.145 M HCI is O…

Q: 6) What is the pH of an aqueous solution that is 0.1M NHẠC1? The Kb value for NH3 is 1.8 x 10-5…

A: Given Kb for NH3 = 1.8 * 10-5. The two ionization reactions are as follows: NH4Cl -------> NH4+ +…

Q: Q3/ Calculate the pH of a solution containing (0.1 M) of (Fe+] [Mg+]. knowing that Ksp is for…

A: Dissociation of Fe(OH)3 : Fe(OH)3 → Fe3+ + 3 OH- Ksp = 1 x 10-13 = [Fe3+] [OH-]3 Dissociation of…

Q: 27.) If an HA is 0.15 M in an aqueous solution of the weak acid at 25.0°C with a pH of 5.35, the Ka…

Q: Part C For 260.0 mL of a buffer solution that is 0.2922 M in CH3 CH,NH, and 0.2677 Min CH3CH2NH3CI,…

A: The buffer solution contains C2H5NH2 (weak base) and C2H5NH3Cl (salt of strong acid and weak base).…

Q: Ex. What is the Acetic acid concentration needed to prepare a buffer solution with pH= 4.32, if the…

A: Henderson's equations enable the calculation of the pH of buffer solutions prepared by mixing known…

Q: The Ka for benzoic acid is 6.5 10-5. Calculate the pH of a 0.10 M benzoic acid solution.

A: Benzoic acid is a weak acid so it will not completely be dissociated in its aqueous solution.…

Q: Ihave some acetic acid that dissociates in water. [CH3COOH] = 0.405 M and [CH3COO]=0.505 M.…

A: The acid ionization constant for acetic acid is 1.8×10 -5.

Q: QUESTION 5 a) Calculate the pH of a solution when 0.025 mol of benzoic acid, CH-COOH is mixed with…

Q: If this picture is still unclear, please take my word for it, there is no more information besides…

A: Aspirin is a weak acid. It undergoes dissociation as:HA -----> H+ + A-The dissociation constant…

Q: QUESTION 2 Choose the correct acid ionization constant (ka) expression for hydrochloric acid. Hint:…

A: The chemical equation for the ionisation, HCl (+H2O) -----> H3O+ + Cl- Therefore, Ka = [H3O+]…

Q: PH value 9.45 using 0.3 M Na2CO3 and 0.2 M HCl How much of each solution to prepare the 1 L buffer…

A: Solution:

Q: ph of a 30.0 ml sample of 0.1 M HOAc is 3.22, what's the equilibrium [H+] and the Ka value?

A: Given :- pH is 3.22 of a 30.0 mL sample of 0.1 M HOAc. To calculate [H+] & Ka value. Now, HOAc…

Q: What is the pH of a 80.0 mL solution which is 0.27 M in IO¯ and 0.41 M in HIO? The Ka for HIO is 2.3…

A: 1- First calculate the pKa value of acid HIO : We know that, pKa = -log(Ka) pKa = -log( 2.3 ×…

Q: What is the pH of a solution prepared by adding 0.025 mol of NaOH to 400. mL of 0.10 M C6H5COOH? Ka…

A: 0.025 mol of NaOH is added to 400 mL of 0.10 M C6H5COOH. The reaction taking place is, C6H5COOH +…

Q: Calculate the expected pH of a buffer prepared by dissolving 1.3 mols of acetic acid and 0.4 mols of…

A: Given buffer solution pH calculated by using formula.

Q: 1. 0.02 mole of HCl is added to one liter of buffer containing 0.05 mole of NH,OH and 0.03 mole of…

A: Moles of NH4 OH = 0.05mol Moles of NH4 Cl =0.03 mol Moles of HCl is 0.02 mol Now, NH4 OH + H+…

Q: What is the pH of an aqueous solution that is 0.1M NHẠC1? The Kb value for NH3 is 1.8 x 10-5 (Hint:…

A: Since NH4Cl is completely soluble in water, it is dissociated into NH4+(aq) and Cl-(aq). NH4+(aq) is…

Q: What is the pH of a buffer solution that is 0.192 M in HX (weak acid) and 0.155 M in Nax (conjugate…

Q: Q1//A solution of 0.1 M of BX salt with pH=9.5, the HX is weak acid and BOH a strong base. Calculate…

Q: (Hand by written ans.)1. A buffer solution was prepared by dissolving 0.15 mol of sodium ethanoate…

A: here we are required to find the change in pH when 1.0 ml of 1.0 mol /L hydrochloric acid is added…

Q: QUESTION 11 How many mL of 0.588 M NaOH is needed to titrate 25.0 mL of 0.587 M H2SO4 to the…

A: The volume of NaOH is calculated below.

Q: 1. A buffer solution is 0.347 M in CH3COOH and 0.207 M in CH3COOK. If Ka for CH3COOH is 1.8×10-5,…

A: In the Question-1 we will determine the pH of the buffer solution. How we can determine the pH of…

Q: What is the ratio of base to acid required to create a buffer system using nicotine (C10H14N2, K…

A: Given data Kb of nicotine (C10H14N2) =1.00×106 pH of the buffer solution = 9.2

Q: chemist titrates 130.0mL of a 0.6404M acetic acid (HCH3CO2) solution with 0.7306M NaOH solution at…

A: Titration between weak acid and Strong base :

Q: app.101edu.co Question 5 of 9 In a titration of 49.0 mL of a 0.500 M solution of a diprotic acid…

A: Given that: [H2C3H2O4] = 0.500M Volume = 49.0mL = 49.0mL×1L/1000ml = 0.049 L Molarity = moles ÷…

Q: What is the pH of the solution that results from mixing 25 mL of 2.60x10-2 M NH3 and 25 mL of…

Q: Case 3: pH with known K: The dissociation of ammonia (NH3) in water is shown below: NH3 (aq) + H2O…

Q: Suppose you titrate NH3 with HC1. With 25.00 mL of NH3 in the flask, it takes 25.00 mL of 0.100 M…

A: Given, Volume of NH3 in flask = 25.00mL. Volume of HCl = 25.00mL. Molarity of HCl = 0.100M. The…

Q: Calculate the pH of an aqueous solution that is 3.24 x 10-1 M oxopropanoic acid and 0.101 M sodium…

A: A buffer solution is a type of solution which can resist the pH change when small amount of acid or…

Q: A 35.0mL solution 0.15M pentanoic acid(Ka = 6.30x10) is titrated 0.25M KOH. What is the pH after…

Q: The pH of a blood plasma is 7.36. Assuming the principle of buffer system is HCO3-/H2CO3, calculate…

A: This HCO3-/H2CO3 that is carbonate-bicarbonate buffer having pH 9.2 to 10.6 are used in many protein…

Q: Q1//A solution of o.1 M of BX salt with pH=9.5, the HX is weak acid and BOH a strong base. Calculate…

A: Use pH formula, used to calculate the pH of salt formed by weak acid and strong base to find the…

Q: What is the pH created when 2.600 L of an aqueous weak monoprotic acid whose molarity is 0.1750 M…

Q: I need to find the pH of this weak acid and strong acid solution. I set up an ICE table with the…

A: Dissociation of strong acid such as HNO3 is 100%. Dissociation of weak acid such as HC6H5O is only…

Q: weak acid has a Ka value of 4.68 x 10-6. If [HA] = 0.004 and [A-] = 0.0076, what is the pH of the…

A: We can used Henderson equation for determination of pH of a buffer solution. Equation is : pH = pKa…

Q: A solution of acid HA (0.030 M) was found to have [H*]= 6.5 x 104 M. Calculate the Ka value for the…

Q: A.) The value of Ka for hydrocyanic acid is 4.00×10-10. What is the value of Kb, for its conjugate…

A: A. We have to calculate the Kb for its conjugate base. B. We have to calculate the Ka for acid.

Q: 25.00 mL of a 0.22M C6H5COOH( KA = 6.3x10-5) is titrated with a 0.15 M NAOH solution. What is the pH…

A: “Since there are multiple questions and it is not mentioned that which one has to be solved so I am…

Q: Calculate the Kb of a 0.01M NH4OH with a hydroxide concentration of 0.005M. ka is 5x10-3

A: Kb of weak base The base dissociation constant of a weak base is the constant on reaction with…

Q: The acid-dissociation constant of hydrocyanic acid (HCN) at 25.0°C is 4.9 × 10-10. What is the pH of…

A: Given, Concentration of the sodium cyanide (NaCN) solution = 0.080 M Acid dissociation constant…

Q: Chem101 app.101edu.co Question 19 of 23 Submit What is the pH of a 0.820 M solution of Ca(NO2)2 (Ka…

Concept explainers

Introduction to chemistry

Chemistry is a branch of science that deals with the analysis of material and the substances that comprise it. It also manages the properties of these substances and their reactions to form new substances. It is basically centered on particles and atoms that make up components and mixtures. These chemical species will in general connect using bonds.

Question

Question attached

Calculate the acetate ion concentration in a solution prepared by dissolving 6.20x10-3 mol of HCI(g) in 1.00 L of 1.20 M aqueous acetic acid (Ka = 1.80x10-5).
mol/L
Submit Answer
Tries 0/5
Calculate the pH of the above 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 3

VIEW

Step by step

Solved in 3 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

When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
Sketch a titration curve for the titration of potassium hydroxide with HCl, both 0.100 M. Identify three regions in which a particular chemical species or system dominates the acid-base equilibria.
What is the pH of a solution made by combining 157 mL of 0.35 M NaC2H3O2 with 139 mL of 0.46 M HC2H3O2? The Ka of acetic acid is 1.8 × 10-5
What is the pH of a solution made by mixing 30.00 mL of 0.10 M acetic acid with 40.00 mL of 0.10 M KOH? Assume that the volumes of the solutions are additive. Ka = 1.8 × 10-5 for CH3CO2H.
Acetic acid has a Ka of 1.8 x 10-5. Calculate the pH at the point when 30.00 mL of 0.150 M NaC2H3O2 is has been mixed with 37.2mL of 0.125 M HBr.
Calculate the pH and [H3O+] of a solutio n prepared by dissolving 0.25mol of NaC2H3O2 in 500. mL of 0.10 M HC2H3O2.Ka HC2H3O2 = 1.80 x 10-5
2. The ionization constant for acetic acid is 1.8 x 10-5. How many grams of NaC2H3O2 must be added to one liter of a 0.20 M solution of HC2H3O2 to maintain a hydrogen ion concentration of 6.5 x 10-5 M?
Calculate the percent ionization of Ammonium hydroxide, NH4OH at the following concentrations: (a) 0.60 M, (b) 0.0046 M, (c) 0.00028 M. Comment on the trends. A 0.040 M solution of a monoprotic acid (HA) is 14% ionized. Calculate the ionization constant, Kc of the acid. (a) Calculate the percent ionization of a 0.20 M solution of the monoprotic acetylsalicylic acid (aspirin) for which Ka = 3.0 x 10-4 .(b)The pH of gastric juice in the stomach of a certain individual is 1.00. After a few aspirin tablets have been swallowed, the concentration of acetylsalicylic acid in the stomach is 0.20M. Calculate the % ionization of the acid under these conditions. What effect does the nonionized acid have on the membranes lining of the stomach? Calculate the [H+], [C2O4-2], and [H2C2O4] in a 0.0010M H2C2O4 (Ka = 5.4 x 10-2)
what is the pH of a solution that contains 0.75 M acetic acid (Ka= 1.8x10-5 ) and 0.50 Msodium acetate?
A solution of volume 0.500 L contains 1.68 g NH3 (Kb = 1.8 x 10^-5) and 4.05 g (NH4)2SO4. How many milliliters of 12 M HCI must be added to 0.500 K of the original solution to change its pH to 9.00?
What is the hydronium-ion concentration in a solution resulting from mixing 133 mL of 0.100 M HCN and 80 mL of 0.100 M KOH at 25°C? Ka for HCN = 4.9 × 10-10 at 25°C
Calculate the pH of a solution that is 0.155 M in acetic acid and 0.255 M in sodium acetate. The Ka of acetic acid is 1.8 x 10^-5.