Answered: What is the pH of a 0.050 M solution of…

Science

Chemistry

What is the pH of a 0.050 M solution of formic acid?

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 96QRT

See similar textbooks

Related questions

Q: Find the pH of a solution 2.0 M in ethylamine CH3CH2NH2. For CH3CH2NH2 Kb=5.6x10-4. Explain step by…

Q: A 0.10 M solution of formic acid (HCOOH) is prepared in various solvents: (a) 0.10 M Ca(HCOO)2…

A: The given data contains, Molarity of HCOOH = 0.10 M Molarity of Ca(HCOO)2 =0.10 M Ka = 1.78 X 10-4

Q: Predict the position of equilibrium and calculate the equilibrium constant, Keq, for each acid-base…

A: The reaction between methyl amine and acetic acid gives methyl ammonium ion and acetate ion. But the…

Q: 0.92 M

A: From Henderson equation we know that pH = pKa + log [salt] / [acid ] ............ (1)

Q: Label acidic basic or neutral: (you will first need to find the pH) 3.9 x 10^-8M NaOH

Q: The Kb of methylamine is 4.4 x10-4. What is the pH of a 0.35 M solution of methylamine? 11.56…

A: Arrhenius theory of electrolytic dissociation assumes that a dynamic equilibrium exist between ions…

Q: What is the ratio of concentrations of acetate ion and undissociated acetic acid in a solution that…

A: Ethanoic acid is a weak acid and the dissociation of acetic acid is given by: CH3COOH ⇌ CH3COO-…

Q: In an equation of hydrofluoric acid plus water yields fluoride ion plus hydronium ion, What is the…

Q: What is the pH of a 0.020M ammonia (NH3) solution if its Kb value is 1.8x10-5? a.12.3 b.10.8 c.3.2…

A: Given : [NH3] = 0.020 M Kb = 1.8×10-5 pH = ?

Q: Calulate the pH of each of the following: 0.05M HCl 0.06M NaOH 0.06M CH3COOH (ka = 1.8 x 10-5…

Q: Calculate the pH of a 0.202 M aqueous solution of triethanolamine (C6H15O3N, Kb = 5.8×10-7) and the…

Q: In a solution prepared by dissolving 0.100 mole of propanoic acid in enough water to make 1.00 L of…

Q: Determine the conjugate base/acid of each (with solution). What strong base can deprotonate the…

A: Concept is based on Conjugate acid-base pair.

Q: Directions: Write the correct Lewis structure and show the step-by-step solution on how you came up…

A: The concept of covalent bond is explained Lewis. The atoms achieve stable octet configuration when…

Q: Calculate the pH of a 0.0470 M aqueous solution of the weak base methylamine (CH3NH2, Kb =…

Q: Salicylic acid, HOC6H4CO2H, and its derivatives have been used as pain relievers for a long time.…

Q: Calculate the pH of a 1.00L solution which is made up of 0.058 mol acetic acid and 0.030 mol sodium…

A: 1- First calculate the pKa of acetic acid : pKa = -log(Ka) pKa = -log( 1.8 × 10-5 ) pKa = 4.74

Q: Amphetamine (C9H13N) is a weak base with a pKb of 4.2. Calculate the pH of a solution containing an…

A: Given, pKb = 4.2 Concentration of amphetamine (C9H13N) = 230 mg/L So, there is 230 mg of…

Q: Label acidic basic or neutral: (you will first need to find the pH) 1.0 x 10-4 M HBr

Q: What is the pH of a solution containing 0.30 M CH₃COONa and 0.10 M CH₃COOH? The Ka of CH₃COOH is 1.8…

Q: CHM 1360 Lab 1 Buffers Worksheet Type your…

A: 1. The Lewis dot structures of acetic acid and acetate: There is only one acidic hydrogen in an…

Q: Calculate the pH of a solution that is 0.112 M in sodium formate (NaHCO2) and 0.266 M in formic acid…

A: The given information is: Conc. of sodium formate (NaHCO2) = 0.112 M Conc. of formic acid (HCOOH) =…

Q: why, during an experiment, was the initial pH of HCl, a strong acid, 2.12, while the weak acid,…

A: During an experiment, the initial pH of HCl, a strong acid, 2.12, while the weak acid, acetic acid,…

Q: beginning with arecoline (pKa:7.6), Show the acid dissociation equilibrium reaction for arecoline in…

A: Structure of arecoline:

Q: Which of the following acids has the weakest conjugate base? Chlorous acid, Ka = 1.1 x 10-2…

A: The strongest an acid , the weakest is its conjugate base. The acid which has highest Ka value is…

Q: Calculate the pH of a 0.035 mol dm–3 solution of ethanoic acid (assume that the degree of…

A: In given question dissociation constant of ethanoic acid is used.

Q: A 0.763 M solution of a weak acid (HA) is made. The solution has a pH of 5.32. Calculate the Ka of…

Q: When HBr reacts with equal moles of CH3NH2 is the resulting solution is Neutral Acidic Basic…

A: Substances that can liberate hydronium ions in solution is called an acid and those that release OH-…

Q: Calculate the pH of a 0.600 M solution of methylamine CH3NH2. Kb = 4.4 x 10–4

A: CH3NH2 is a base and CH3NH3+ is its conjugated acid. pKb of CH3NH2 is 4.4×10-4. Expression for Kb is…

Q: The pH of a 1.4M solution of 3-hydroxypropanoic acid (HC₂H₂O3) is measured to be 2.18. Calculate the…

A: Given-> Concentration of 3-hydroxypropanoic acid = 1.4 M pH = 2.18

Q: Using their Ka values, what is the pOH of 0.10 M mandelic acid 0.10 M maleic acid 0.10 M malonic…

A: Ka = [H+][A-]/[HA] .....................(i) [H+] is the concentration of the proton…

Q: Identify the following species: Strong Acid Strong Base Weak Acid Weak Base Salt CaBr2 Strong Acid…

A: The species that donate a proton is known as acid and the species that gains a proton is base.…

Q: Calculate the pH of a 0.105 M solution of ethylenediamine (H,NCH,CH,NH, ). The pKa values for the…

Q: Classify K2O strong acid weak acid strong base weak base

A: Acid- The species which is able to donate H+ ion is called as acid. Bade The species which is able…

Q: What is the pH of a solution with 0.46 M lactic acid and 0.07 M sodium lactate? Include 3 sig figs…

Q: Which pH change represents a ten fold decrease in the concentration of H3O+? (1) pH 5 to pH 7…

Q: Label acidic basic or neutral: (you will first need to find the pH) 2.0 x 10^-6 M HBr

A: We have given that Molarity of HBr = 2.0×10-6 M We know that The pH of a solution is a measure of…

Q: If the pH of a 0.050 M solution of the acid HX is 2.0 and the pH of a 0.050 M solution of the acid…

A: Given : Concentration of HX = 0.050 M pH of HX solution = 2.0 Concentration of HY = 0.050 M And pH…

Q: Complete and balance the acid-base reaction. Identify the acid, base, conjugate acid and conjugate…

A: According to Bronsted-Lowry concept, the acidic and basic character of a compound can be interpreted…

Q: For equal concentrations of acids such as hydrofluoric acid, acetic acid, and benzoic acid, does the…

A: Ka is the dissociation constant of an acid. For example, the dissociation of HCl can be written as…

Q: hydronium-ion concentration of a 2.13 ✕ 10−4 M solution of p-bromobenzoic acid, BrC6H4COOH, for…

A: Degree of dissociation is the number of moles dissociated per unit concentration of any electrolyte.

Q: Chemistry beginning with arecoline (pKa:7.6), Show the acid dissociation equilibrium reaction for…

Q: Using the Henderson-Hasselbach equation predict under which of the following conditions will the pH…

A: pH= Pka + log([Salt]/[Acid]) so pH > Pka when log term is greater that Zero so in that case…

Q: Calculate the pH of a 1.00L solution containing 10.0mL of 5.0M acetic acid and 29.0mL of 0.3M sodium…

A: Acetic acid and sodium acetate form a buffer solution. The pH can be calculated using the…

Q: Given the following data, Base K, NH3 1.8 x 10-5 CH3NH2 5.0 x 10 C6 H6 NH2 4.2 × 10-10 Calculate the…

A: Hey, since you have asked multiple question, we will solve the first question for you. If you want…

Q: Using the Henderson-Hasselbach equation predict under which of the following conditions will the pH…

A: The Henderson–Hassel balch equation is used to calculate the amount of acid and conjugate base to be…

Q: Indicate whether an alcohol (ROH) with a pKa value of 15 has more charged or more neutral molecules…

A: An acidic substance is the substance that can give H+ ions. They are corrosive and sour in nature.…

Q: ROUND YOUR ANSWER TO 3 SF ONLY Calculate the pH change that occurs when 1.00 g of NaOH is added to…

A: (1) Initially, calculate the pH of the NH3 solution. The ICE table for the NH3 solution is expressed…

Q: A certain organic amine acts as a mono acid base in an aqueous solution. A 0.05M solution has a…

Q: What concentration of formic acid will result in a solution with pH=1.90? The value of Ka for formic…

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

What is the pH of a 0.050 M solution of formic acid? Assume that you have two unlabeled bottles, one of which contains phenol (pKa = 9.9) and one of which contains acetic acid (pKa = 4.76). In light of your answer to the previous question, suggest a simple way to determine what is in each bottle.

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

Find the value of Kb for the conjugate base of the following organic acids. (a) picric acid used in the manufacture of explosives; Ka = 0.16 (b) trichloroacetic acid used in the treatment of warts; Ka = 0.20
Given that acetic acid has Ka = 1.8 x 10–5, what is the pH of a solution that contains the molar ratio of conjugate base-to-acid: [CH3CO2–]/[CH3CO2H] = 1/10?
beginning with arecoline (pKa:7.6), Show the acid dissociation equilibrium reaction for arecoline in water. Label conjugate base and weak acid in this reaction. Saliva has a pH of 6.8, Calculate the percentage of arecoline in the HA form in typical saliva. Betel nut is usually chewed with a small amount of slaked lime Ca(OH)2. Explain why slaked lime improves the bioavailability and thus the effects of arecoline.
Chemistry beginning with arecoline (pKa:7.6), Show the acid dissociation equilibrium reaction for arecoline in water. Label conjugate base and weak acid in this reaction. Saliva has a pH of 6.8, Calculate the percentage of arecoline in the HA form in typical saliva. Betel nut is usually chewed with a small amount of slaked lime Ca(OH)2. Explain why slaked lime improves the bioavailability and thus the effects of arecoline.
Propanoic acid, CH3CH2COOH, has a pKa =4.9. Draw the structure of the conjugate base of propanoic acid and give the pH above which 90% of the compound will be in this conjugate base form.
The pH of a 1.1M solution of 4-chlorobutanoic acid (HC4HO₂Cl) is measured to be 2.24. Calculate the acid dissociation constant K of 4-chlorobutanoic acid. Round your answer to 2 significant digits. a K = 0 a 0 x10
The acid dissociation constant Ka of alloxanic acid HC4H3N2O5 is ×2.2410−7 . Calculate the pH of a 3.2M solution of alloxanic acid. Round your answer to 1 decimal place.
Reaction between hydrochloric acid and sodium hydroxide: HCl(aq) + NaOH (aq) → NaCl(aq) + H2O(l) Reaction between acetic acid and sodium hydroxide: CH3COOH(aq) + NaOH(aq) → CH3COONa(aq) + H2O(l) Consider the two reactions you have just written out above. Which reaction would you predict to have higher pH at the equivalence point? Explain your reasoning.
Acid Formula Ka Acetic acid HCH3CO2 1.8*10^-5 hypochlorous acid HClO 3.0*10^-8 Base formula Kb ammonia NH3 1.8*10^-5 aniline C6H5NH2 4.3*10^-10 Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. Solution pH .1 M KCH3CO2 .1 M C6H5NH3Br .1 M NH4Cl .1 M KI
Phenols are aromatic rings with an alcohol functional group attached directly to the ring. These compounds have unique acidity and solubility for alcohol groups. Phenolic functional groups are weak acids. Predict the solubility of the conjugate base of phenol in water.
Indicate whether an alcohol (ROH) with a pKa value of 15 has more charged or more neutral molecules in a solution with the pH values
2-Methylvaleric acid, CH3(CH2)2CH(CH3)COOH has a pKa=4.9. What is the pH of its conjugate base which 90% of the compound will be in in this conjugate base form.