answer all part fast Question:-120-g of benzoic acid is dissolved in 600 mL of water. Calculate the pH of the solution.0.1 moles of acetic acid is dissolved in enough water to make 1 L. What is the pH of thesolution?A weak acid solution of H2CO3 (0.75 M) has a pH of 2. Determine the value of Ka.

Since you have posted multiple questions, we are entitled to answer the first only. 1) Given: Mass…

Answered: 20-g of benzoic acid is dissolved in…

Science

Chemistry

20-g of benzoic acid is dissolved in 600 mL of water. Calculate the pH of the solution.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter15: Complex Acid/base Systems

Section: Chapter Questions

Problem 15.16QAP

See similar textbooks

Related questions

Q: Calculate the pH of an aqueous solution containing acetic acid at an analytical concentration of a.…

A: For aqueous solution of CH3COOH : pKa = 4.74 pH = 0.5 x ( pKa - log C ) (a) C = 3.00 x 10-1 M pH =…

Q: Calculate the pH of a solution that contains 0.25 M benzoic acid (C6H5CO2H) and 0.15 M sodium…

A: Given :- Concentration of benzoic acid = 0.25 M Concentration of sodium benzoate = 0.15 M Ka =…

Q: Calculate the pH of a solution that is prepared by dissolving 7.85 g of lactic acid (90.08 g/mol)…

A: Here we are required to find the pH of solution prepared by mixing lactic acid and sodium lactate.

Q: Sodium hydroxide is used to clear clogged drains. A solution of NaOH has a pH 1 2 of 9.52 at 25C.…

A: Given: The pH of the solution = 9.52

Q: The solubility of Ca(OH)2 at 20°C is 0.165 g/100 g H2O. The density of a saturated solution is 1.000…

A: The solubility of Ca(OH)2 at 20°C is 0.165 g/100 g H2O. The density of a saturated solution is 1.000…

Q: The ionization constant (Kb) of trimethylamine ((CH)3)3N) is 7.40 x 10–5 . If 5.911 grams of…

Q: Calculate the pH of a 2.1 M Ca(OH)2 aqueous solution.

A: Consider the given information is as follows; Molarity of Ca(OH)2 = 2.1 M pH = ?

Q: A chemist dissolves 290. mg of pure potassium hydroxide in enough water to make up 70. mL of…

A: We have to find the pH of solution

Q: The pH of a 0.75 mol/L propanoic acid solution is

Q: A solution is prepared by dissolving 1.600 g of sodium acetate (CH3COONa) into 100.00 mL of a…

A: • pH of weak acid can be calculate by the help of Hendenson - Hasselbalch equation:-pH=pka +…

Q: Calculate the pH of each of the following buffered solutions: 1. 0.10 m acetic acid / 0.25 m…

Q: Calculate the percent ionization and the pH of the following solution of benzoic acid, HC7H5O2 (Ka =…

Q: If 1.00 mol of HCOOH and 0.500 mol of NaHCOO are added to water and diluted to 1.00 L, calculate the…

A: Given: Moles of HCOOH = 1.00 mol Moles of NaHCOO = 0.500 mol Volume of solution = 1.00 L Acid…

Q: Calculate the pH of a solution prepared by dissolving 0.37 mol of formic acid (HCO2H) and 0.23 mol…

A: Given, moles of formic acid = 0.37 mol moles of Sodium formate = 0.23 mol Volume = 1 liter As we…

Q: Calculate the pH of a 0.100 M KCN solution.

Q: What is the pH of a 0.79 M solution of methylamine (CH3NH2, Kb = 4.4 x 10–4) at 25oC?

Q: An acid-base equilibrium system is created by dissolving 0.50 mol CH3CO2H in water to a volume of…

A: The acid-base equilibrium between CH3COOH and H2O is given by the reaction.

Q: Determine the pH of a 0.50-M solution of NH4OCl.

A: The question is based on the concept of salt hydrolysis. we have to calculate pH of the given salt…

Q: An aqueous solution is composed of acetic acid and sodium hydroxide. The acetic acid is 0.155M and…

A: The condition given as mixture of weak acid and strong base ,in which base will react with weak acid…

Q: 2) Determine the pH of a solution by adding 0.23 mole formic acid and 0.17 mole of sodium formate in…

A: Henderson Hasselbalch equation is given by, pH=-log(Ka)+log[salt][acid] where Ka is the acid…

Q: Use Le Chatelier's Principle to qualitatively determine what the pH of a 0.2 M NH4Cl would be…

A: Le Chatelier's Principle : At equilibrium the change in any property like, temperature,pressure and…

Q: When 2.0 x 10-2 mole of nicotinic acid (a monoprotic acid) is dissolved in 350. mL of water, the pH…

A: Nicotine is a weak monoprotic acid so it dissociated in less amount. So we can denotes it by HA .

Q: 0.25 mol of benzoic acid and 0.15 mol of sodium benzoate are dissolved in 1 L of water. What is the…

Q: Calculate the pH of a solution that is 0.520 MM in pyridine (C5H5NC5H5N) and 0.440 MM in pyridinium…

A: Recall the following relation to calculate pH of the given solution…

Q: 20 ml of 0.2 M NaOH solution be treated with 40 ml of 0.2 M acetic acid solution to give 60 ml.…

A: An acidic buffer is defined as an aqueous solution that consists of a mixture of a weak acid and its…

Q: Hydrazoic acid, HN3, has an acid dissociation constant of 2.5 x 10-5. Calculate the equilibrium…

A: Given : Initial concentration of HN3 = 0.0750 M Since HN3 is a weak acid. Hence it will dissociate…

Q: Calculate the pH of 0.0500 M aqueous solution of Methylamine.

A: Concentration of a solution can be measured in terms of molarity, molality and normality.

Q: A chemist dissolves 165. mg of pure sodium hydroxide in enough water to make up 190. mL of solution.…

A: Given, Weight of pure sodium hydroxide = 165 mg = 0.165 g volume of solution = 190 mL = 0.190 L…

Q: Calculate the pH of a 0.50 M solution of sodium formate (NaHCOO) given that the Ka of formic acid…

A: Given, The pH of a 0.50 M solution of sodium formate (NaCOOH) is: The Ka of formic acid (HCOOH) is…

Q: 9) Calculate the pH of 1.5 M solution of hydroxylamine, NH2OH, at 25°C. К, 3D 9.1 х 10

Q: What is the pH of a 0.21 M solution of methylamine

A: Given :- Initial concentration of CH3NH2 solution = 0.21M Kb = 4.4 × 10-4 To calculate :- pH of…

Q: At 25°C, the Ka of pentafluorobenzoic acid (C6F5COOH) is 0.033. Suppose 0.100 mol of…

A: Given, Ka for C6F5COOH = 0.033 moles of C6F5COOH = 0.100 mol Volume of water = 1.00 L pH = Unknown

Q: Calculate the concentration of sodium benzoate (NaC6H5COO) that must be present in a 0.20 M solution…

A: Concentration of benzoic acid = 0.20 M pH = 4 pKa of benzoic acid = 4.20

Q: What do you call an aqueous solution that has a large amount of NH4Cl and NH3 dissolved in it? Write…

A: a solution which resist in pH change value upon addition of small amount of strong acid or base…

Q: Calculate the pH of a solution prepared by dissolving 0.0775 mol acetic acid (HCOOH) and 0.0460 mol…

A: Given-> Moles of HCOOH = 0.0775 mole Moles of HCOONa = 0.0460 mole Volume = 1 L Ka = 1.77 × 10-4…

Q: Calculate the pH of a solution at 25.0 °C that contains 1.94 x 10 -10 M hydronium ions.

A: We have to calculate the pH of solution that contains 1.94 x 10-10 M hydronium ions.

Q: alculate the pH of the glacial acetic acid and the solution you prepared in step 1. Step 1: Glacial…

Q: Determine the pH of a solution by adding 0.23 mole formic acid and 0.17 mole of sodium formate in…

A: Here formic acid is a weak acid and sodium formate is an salt of weak acid so they both combine to…

Q: Calculate the formate ion concentration and pH of a solution that is 0.050 M in formic acid (НСООН,…

Q: A.) What is the pH of a 0.25 M solution of sodium propionate, NaC3H5O2, at 25°C? (For propionic…

Q: Calculate the concentration of hydroxide in the following solutions. Pure water (pH = 7.00) 3 M KOH…

Q: Calculate the pH of the following: 1. 0.10 M 2-aminophenol 2. 0.10 M disodium hydrogen arsenate

A: a) Given: Concentration of 2-aminophenol (which is a base like NH3 and hence assuming it B) = 0.10 M…

Q: Calculate the pH of an aqueous solution of 0.1930 M sodium carbonate. pH =

Q: Calculate the pH of a vinegar solution with an acetic acid HC2H302 concentration of 0.75 M.

Q: 3g of benzoic acid (Molecular mass = 122 g/mol) are dissolved in 100 mL of pure water. Calculate the…

A: Ionization of weak monoprotic acid and pH calculation:

Q: The solubility of Ca(OH)2 at 20°C is 0.165 g/100 g H2O. The density of a saturated solution is 1.000…

A: Assuming we gave 100 g of Ca(OH)2 Since solubility given = 0.165 g / 100 g H2O Hence mass of…

Q: Calculate the percent ionization and the pH of the following solution of benzoic acid, HC7H5O2 (Ka =…

Q: Calculate the pH of the following: 1. 0.10 M 2-aminophenol|

A: Given: Concentration of 2-aminophenol (which is a base like NH3 and hence assuming it B) = 0.10 M

Q: Calculate the pH of a 0.0555 M aqueous solution of the weak base ethylamine (C2H5NH2, Kb =…

A: For C2H5NH2 , Kb = 4.30 × 10-4 C2H5NH2 + H2O ⇌ C2H5NH3+ + OH- Kb = [C2H5NH3+] [OH-] / [C2H5NH2]…

Concept explainers

States of Matter

The substance that constitutes everything in the universe is known as matter. Matter comprises atoms which in turn are composed of electrons, protons, and neutrons. Different atoms combine together to give rise to molecules that act as a foundation for all kinds of substances. There are five states of matter based on their energies of attraction, namely solid, liquid, gases, plasma, and BEC (Bose-Einstein condensates).

Chemical Reactions and Equations

When a chemical species is transformed into another chemical species it is said to have undergone a chemical reaction. It consists of breaking existing bonds and forming new bonds by changing the position of electrons. These reactions are best explained using a chemical equation.

Question

answer all part fast

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

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

2. A 0.0560 g quantity of acetic acid is dissolved in enough water to make 50.0 mL of solution. Calculate the concentrations of H3O*, CH3COO and CH3COOH at equilibrium. What is the pH of the solution? (Ka = 1.8x10-5) — СНCOО- (аq) + НзО* (аq) CH:COOH(аq) a) Calculate the initial concentration of CH3COOH. (C:12; H:1; 0:16) b) Calculate the concentration of CH3COO- (aq) and H3O* (aq) at equilibrium. c) Calculate pH of the solution.
3. The pH of an acid solution is 6.20. Calculate the Ka for the acid. The initial acid concentration is 0.010 M. 4. What is the original molarity of a solution of formic acid (HCOOH) whose pH is 3.26 at equilibrium? 5. Calculate the percent ionization of benzoic acid having the following concentrations: (a) 0.20 M, (b) 0.00020 M. 6. 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. 7. A 0.040 M solution of a monoprotic acid (HA) is 14% ionized. Calculate the ionization constant, Kc of the acid.8. (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.…
A solution is made by dissolving 18.7 g of CH3NH:NO: in 500.0 mL of water. L Does CH.NH:- have any acidic or basic properties? Does NO:- have any acidic or basic properties? Write the acidic equilibrium equation that exists in solution What is the value of Ka for CH3NH₂+? The Kb of CH3NH₂ is 4.4 × 10-4. Determine the pH of the solution.
Two part question In the laboratory, one general chemistry student measured the pH of a 0.590 M aqueous solution of quinoline, C9H7N to be 9.299. Use the information she obtained to determine the Kb for this studentʻs base. Kb(experiment) =__________ While in the laboratory, another chemistry student measured the pH of a 0.590 M aqueous solution of triethylamine, (C2H5)3N to be 12.229. Kb(experiment) =_________
H. | || The percent ionization of chloroacetic acid is less than that of fluoroacetic acid. :*-C-C-ö-H The percent ionizations cannot be compared without knowing the concentrations of the two acids. The structure of haloacetic acids, XCH,COOH (where X is The percent ionizations cannot be compared without knowing the pH of the solution. either F, Cl, Br, or 1), is shown above. The dissociation constants and molar masses of four haloacetic acids are listed in the table below. The percent ionization of chloroacetic acid is greater than that of fluoroacetic acid. Acid pK. K. Molar Mass(g/mol) CLEAR ALL Fluoroacetic acid 2.59 2.57 x 10–3 78.0 Chloroacetic acid 2.87 1.35 x 10–3 94.5 Bromoacetic acid 2.90 1.26 x 10-3 138.9 lodoacetic acid 3.18 6.61 × 10-4 185.9 An aqueous solution contains small but equal concentrations of both chloroacetic and fluoroacetic acids. Which statement comparing the percent ionizations of the two acids in the solution is true? エーO-
butanoic acid is a weak monobasic acid Ka = 6.3 × 10-⁵. a) Calculate the mass of butanoic acid needed to obtain 1 liter of butane acid solution at a concentration of 0.02 mol / liter. b) Calculate [H +] in an acid solution with a concentration of 0.02 mol / liter and calculate the pH of the acid solution in question a)
Chloroacetic acid, HC2H2ClO2, has a greater acid strength than acetic acid, because the electronegativity chlorine atom pulls eloectroms way from the O-H bond and thus weakens it. What is the pH of a 0.045 M aqueous solution of chloroacetic acid? The Ka for HF is 1.3x10-3. You must solve the quadric equation for this problem. Express your answer to two decimal places. -------------------------------------------------------------------------------------------------------------------------- What is the pH of a 0.080 M aqueous solution of methylamine, CH3NH2? The Kb for methylamine is 4.4x10-4. You must solve the quadric equation for this problem. Express your answer to two decimal places.
4G 4:04 Problem Set 8 - Saved CHEMISTRY PROBLEM SET 8 ACIDS AND BASES Answer the following questions. Show your solution(s) to the problem(s). 1. Which of the following does not constitute a conjugate acid-base pair? (a) HNO2, NO2" ; (b) H2CO3, CO32; (c) CH3NH3* , CH3NH2 2. Calculate the pH of a 1.8 x10-2 M Ba(OH)2 solution. 3. Which is more acidic: a solution where [H*] 2.5x10-3 M or a solution with a pOH = 11.6? 4. The pH of a 0.060 M weak monoprotic acid, HA is 3.44. Calculate the Ka of the acid. 5. Calculate the pH and percent ionization of hydrofluoric acid at these concentrations: (a) 0.60 M, (b) 0.080 M, (c) 0.0046 M, (d) 0.00028 M. Comment on the trend. 6. Identify the Lewis acid and Lewis base in the reaction: Co** (aq) + 6NH3(aq) = Co(NH3);* (aq)
4. What is the original molarity of a solution of formic acid (HCOOH) whose pH is 3.26 at equilibrium? 5. Calculate the percent ionization of benzoic acid having the following concentrations: (a) 0.20 M, (b) 0.00020 M. 6. 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. 7. A 0.040 M solution of a monoprotic acid (HA) is 14% ionized. Calculate the ionization constant, Kc of the acid.8. (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?9. Calculate the [H+], [C2O4-2],…
solve a,b,c,d and e. The active ingredient in aspirin is acetylsalicylic acid (HC9H7O4), which has a Ka of 3.00 x 10-4. A 325-mg tablet of aspirin is dissolved in 25.00 mL of water, and the solution is titrated with 0.0500 M NaOH. a) Calculate the initial pH of the aspirin solution. b) What is the pH of the solution after 10.0 mL of NaOH is added? c) How many mL of NaOH are required to reach the equivalence point? d) What is the pH of the solution at the equivalence point? e) Make a rough sketch of the titration curve for this titration. Label the buffer region and the equivalence point.
How many grams of NH4Cl (53.49 g/mol) must be dissolved in 0.639 L of solution in order to obtain a solution that has a pH equal to 4.79? The Kb of NH3 at the temperature in this problem is 3.2 × 10-5. The Kw can be assumed to equal 1.0 x 10-14. Please note that the solution (the underlined part) is not explicitly named, neither its concentration is given.
1.) In a 0.100M aqueous solution of a weak acid, the acid is 3.7% dissociated. What is the Ka for this acid? 2.) What is the pH of a 0.010M solution of pyridine, C2H5N, a weak base? It's Kb is 1.5x10-9. 3.) Calculate the pH and percent ionization of a 15.0 M solution of a weak base. (pKa=9.26) SHOW ALL WORK!!