Ethylamine (C2H5NH2) has a Kb value of 4.5x10–4. Calculate the pH of a buffer solution that is 0.00298 M ethylamine and 0.00546 M ethylammonium chloride.

Q: If the concentration of the weak base ammonia is 0.10 M and it is titrated with 0.1 M HCl, and the…

A: pH of a basic buffer solution can be calculated as follows:

Q: 1,2-diaminoethane, H2N-CH2-CH2-NH2, is used extensively in the synthesis of compounds containing…

A: since you have posted multiple questions in a single session we are entitled to answer only first…

Q: Hydroxychloroquine is a weak Bronsted base.

A:

Q: In aqueous solution, pentanoic acid (HC-H,02) dissociates to produce its conjugate base, the…

A:

Q: Calculate the pH of a 1.01×10-2 M solution of the decongestant ephedrine hydrochloride if the pKb of…

A: Given:Molarity = 1.01×10-2 MpKb of ephedrine = 3.86we need to Calculate the pH.

Q: Calculate the pH and concentrations of CH3NH2 and CH3NH+3 in a 0.0341 M methylamine (CH3NH2)…

A: The given data contains, Concentration of methylamine = 0.0341 M. Kb of CH3NH2 is 4.47×10−4.

Q: Calculate the pH at 25°C of a 0.45 M aqueous solution of oxalic acid (H2C2O4). (Ka1 and Ka2 for…

A: We have to calculate the pH value.

Q: Write the expresson for the dissociation constant, Ka for an aqueous solution of butanoic acid.…

A:

Q: Calculate the pH of a 0.0500M solution of phenylacetic acid, C6H5CH2COOH and  0.0200M with its salt,…

A: Given,  The pH of a 0.0500M solution of phenylacetic acid, (C6H5CH2COOH) and  0.0200M of its salt,…

Q: n the laboratory, a general chemistry student measured the pH of a 0.354 M aqueous solution of…

A: Here we have:Concentration of diethyl amine = 0.354 MKb= 6.9 × 10-4

Q: that is 0.192 M in lactic acid and 0.155 M in sodium lactate? The Kaof lactic acid is 1.4 × 10-4.…

A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid

Q: Find the pH of a 0.065 M solution of formic acid. The acid dissociation constant (Ka) for formic…

A:

Q: The pH of a solution that is 0.5 in MA and 0.3 in HA is 5.40; determine the pKa of the acid.

A:

Q: What is the pH of a 0.0830 M solution of methylamine (CH₃NH₂, Kb = 4.4 × 10⁻⁴)?

A:

Q: What is the pH of a 1.75 M solution of KX (Kb of X is 1.22 x 10°) (Please show the final result with…

A: Answer:  9.66 Weak base can't dissociate completely, it's  pOH = 1/2 (PKb - logC)

Q: The simplest amino acid is glycine ( molar mass = 75.1 g/mol), whose structure is shown above. An…

A: molarity = ωGmω × 1000V(mL)Given weight of glycine = 0.329 g                                V = 150…

Q: Using the table of the weak base below, you have chosen Pyridine as your weak base in the buffer…

A: Given: Kb of pyridine = 1.7×10-9

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

A:

Q: Calculate the Kb values for the CO32- and C2H3O2- ions using the Ka values for HCO3- (4.7 x 10-11)…

A: We have to find Kb values for the CO32- and C2H3O2- ions using the Ka values for HCO3- (4.7 x 10-11)…

Q: Calculate the pH of the following solutions:1) 0.0624 molar piperazine 2)A 0.0850 molar solution of…

A:

Q: For a weak acid with a pKa of 6.0, show how you would calculate the ration of acid to salt at pH 5.

A:

Q: Which of the following is correct concerning the base ionization constant, Kp, of dimethylamine,…

A: Ionization of amine is water.

Q: Given the pK, of formic acid is 3.74, calculate the pH of a buffer solution that contains 0.10 M of…

A:

Q: What is the pH of a 0.050 M triethylamine, (C2HS)3N, solution? Kb for triethylamine is 5.3 x 10-4

A: We should know that the amine us a basic Compound that will dissociate in solution to give basic…

Q: Oleic acid (which can be denoted as HOL), is a weak acid. Considering its sodium salt, sodium oleate…

A: We have to calculate the pKa of the HOL.

Q: Čalculate the molar concentration of ÕH- in a 0.050 M solu- tion of ethylamine (C2H;NH2; Kp, the pH…

A:

Q: Galaulate the PH and the Pott FOR 9.6M solution OF MH₂ инз K. FOR NH3=1.97105

A: Here we are required to find the pOH and pH of 0.6M of ammonia solution

Q: The pH for 0.0850 M solution of C6H:CH2COOH is 2.68. Determine the value of Ka for CsHsCH2COOH. PREV…

A:

Q: Calculate the pH of 0.564 M HC2H3O2 (Ka of HC2H3O2 = 1.8 x 10-5)

A:

Q: What is the ratio of conjugate base to undissociated acid for a weak acid with a pk, of 4.4 at a pH…

A: Given :  pKa = 4.4  pH = 9  To determine :  Ratio of conjugate base to weak acid

Q: The ionization constant, Ka, for benzoic acid is 6.28 x 105. What is the pK, of this acid? a. 1.59 x…

A: Benzoic acid [C6H5COOH] is a monoprotic weak acid, in solution it partially ionizes and gives an…

Q: Calculate the pH of a solution that is prepared by dissolving 0.470 mol of hydrocyanic acid (HCN, K,…

A: Given- HCN= 0.470 mole HC9H7O4 = 0.164 mole Volume of solution = 3.00 L Ka of HCN = 6.17 x 10-`10 Ka…

Q: A particular solution is 0.05M with respect to ethanoic acid and 0.2M with respect to sodium…

A:

Q: Using the table of the weak base below, you have chosen Aniline as your weak base in the buffer…

A: Given: Buffer solution of weak base aniline (assuming B) and its conjugate acid HB+. pH of solution…

Q: The p Kp of ethylamine is An analytical chemist is titrating 195.8 mL of a 0.6200 M solution of…

A: Given that: Volume of of ethylamine (C2H5NH2) solution = 195.8 mL = 0.1958 L, Molarity = 0.6200 M…

Q: A 1.083 g sample of N-2-acetamido-2-aminoethane-sulfonic acid potassium salt (ACES K*, MW = 220.29…

A:

Q: What is the pH of a solution that contains 0.135 M HCOOH and 0.215 M HCOONa? The pKa of formic acid…

A: pH of the solution is equal to the negative logarithm of hydronium ion while pOH is equal to the…

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: The base protonation constant K of azetidine (C²H²NH) is 1.5 × 10¯8. Calculate the pH of a 0.39 M…

A: The base protonation constant Kb of azetidine C3H6NH is 1.5 × 10-8 .We have to calculate the pH of…

Q: CH3NH2 is a weak base (Kb = 5.0 x 10-4 ) and so the salt CH3NH3NO3 acts as a weak acid. What is the…

A:

Q: What is the pH of a 0.639 M solution of lactic acid? The pKa of lactic acid is 3.854.

A:

Q: Calculate the pH of a 0.300 M solution of the dibasic compound piperazine, which we will designate…

A: pH is used to determine the concentration of hydronium ion.

Q: A 2.5 M solution of formic acid (HCOOH) has a pH of 1.67. What is the pK, of the formate ion…

A: Welcome to bartleby ! We have to calculate pKb

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

A:

Q: What is the pH of a 0.120 M solution of aniline (C6H5NH2, Kb = 4.3 x 1010)?

A: Given: Concentration of aniline = 0.120 M Kb of aniline = 4.3×10-10

Q: Calculate the isoionic pH of 6.022 x 1021 molecules of thereonine in 500 mL of solution. (For…

A:

Q: If the pH value of an aqueous solution of trimethylamine [(CH3) 3N] is 10.75, what should be the…

A:

Q: Calculate the pH of a 27 mg/L solution of hydrocyanic acid (HCN). The pKa of hydrocyanic acid is…

A: Given: The concentration of hydrocyanic acid is 27 mg/L. The pKa of hydrocyanic acid is 9.3.

Q: A 250.0 mL sample of 0.4375 M aniline, C6H5NH2 (Kb = 3.8 x 10-10) reacted with 2.250 L of gaseous…

A: The chemical reaction may be represented as: C6H5NH2+HCN↔C6H5NH3++CN-         --------(1)

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.