What is the% hydrolysis of the acetate ion in a 0.1M solution of CH3COO (NH4) compared to the% hydrolysis of the acetate ion in a 0.1 M solution of CH3COONa. Determine the pH of the final solutions

Q: Calculate the pH of a solution in which [OH−]=7.1×10−3M.

A: The pH of a given solution can be termed as a measure of its basicity or acidity. It is a measure of…

Q: . Strychnine, C,H„N‚O, (aq) is a weak base but powerfully toxic. (a) Calculate the pH of 0.001 mol/L…

A: Given: Concentration of weak base (assuming B) = 0.001 M And Kb of base = 1.0 × 10-6

Q: Determine the pH and equilibrium concentrations of all species of a 25 M H2SO3 solution at 25oC

A:

Q: What is the pH of a 0.0023 mol/L solution of nitric acid? The answer should be to the proper number…

A: pH of the solution is calculated as  pH = – log[H+] Given that [HNO3] = 0.0023 mol/L

Q: Calculate the pH of a 0.008 M nitric acid (HNO3) solution.

A: We know that, HNO3 is a strong acid so completely dissociated. Thus, concentration of [H+]=0.008M

Q: Determine the pH of a 0.20M CH3NH3I solution.

A: Given that: [CH3NH3I] = 0.20M  CH3NH3I is salt made up of weak base CH3NH2 and strong acid HI.

Q: Write the whole acid base equation for the reaction of KOH(aq) with HC4H7O2(aq) b) write the net…

A: (a) Acid base equation  KOH(aq)    +    HC4H7O2(aq)    → KC4H7O2(aq)  + H2O (l)   (b) Net ionic…

Q: For sulfuric acid, K >> 1 and K is 0.012. Calculate the pH of a 1.2 M solution of HSO.

A: Assuming the solution is H2SO4

Q: What is the pH of a 0.590 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

A:

Q: Write the formula of the conjugate acid of CH3CO2H

A: We have to tell the conjugate acid of CH3COOH

Q: Estimate the pH of a 0.016 aqueous lead(ll) chloride

A: Hydrolysis of PbCl2 can form a weak base, Pb (OH) 2 and Cl- that does not combine with H+ as HCl is…

Q: Calculate the pH of the solution, where the acetic acid is x10 stronger than acetate.

A: In chemistry, pH is defined as the potential of hydrogen ion. It is the negative logarithm of…

Q: A 0.54 M solution of chloroacetic acid, CICH2 CO2H, has a pH of 1.57. Calculate K, for the acid. %3D

A: Given: The molarity of the solution of chloroacetic acid = 0.54 M The pH of the solution = 1.57 We…

Q: HC2H3O2

A: Calculate the concentration of hydrogen ions released from the acetic acid. If the concentration of…

Q: Determine the pH of a 0.13 M solution of pyridinium nitrate (C5H5NHNO3) at 25°C. [Pyridinium nitrate…

A: Determine the pH of a 0.13 M solution of pyridinium nitrate

Q: How many moles of nitric acid would you have if you had 0.550 L of a 0.025 M nitric acid solution?…

A: The number of moles of nitric acid (n) is calculated as shown below where M is the concentration of…

Q: calculate the pH of the solution eith an H+1 concentration of 2.90×10-12 and identify the solution…

A: Given,  The concentration of H+ = 2.90 × 10-12 M The pH of the solution is:

Q: Calculate the pH of a 0.125 M sodium propionate (NaC3H5O2) solution

A:

Q: Calculate the pH of (a) 0.10 M NH4CI(aq), (b) 0.25 M NaCH3CO2(aq), (c) 0.200 M CH3COOH(aq).

A: (a) 0.10 M NH4Cl(aq) The reaction is as follows,

Q: Write an ionic equation to represent the hydrolysis of the pyridinium ion, and calculate the pH of…

A: given concentration of C5H5NH+Cl- = 0.0482 M  Kb  for prydine = 1.7× 10-9  Ka  = Kw /Ka   Kw =…

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 solution that is made by dissolving 5.54 g NH4NO3 in enough water to create…

A: First to calculate morality Then to calculate degree of dissociation.  Then to calculate pH.

Q: Calculate the pH of a 0.633 M NH, solution. NH, has a Kp 1.8 x 10–5.

A:

Q: Calculate the pH of an aqueous solution at 25⁰C that is (b) 0.035 M in HClO4 (c) 1.5×10-6 M in HCl.

A: PH = -log [H+]  HClO4 and HCl are strong acid so concentration of H+  ion  concentration..

Q: a) Calculate [H3oʻ], [C2H3O2¯ ] and [HC2H3O2] for a solution prepared by mixing 35.0 mL of o.10 M…

A: The number of moles of acetic acid in 35.0 mL of 0.10 M acetic solution and the number of moles of…

Q: Calculate the pH of a solution that is 0.052 M in HCl and 0.020 in HClO4

A: Given that,  The concentration of the solution in HCl = 0.052 M And the concentration of the…

Q: Determine the pH of the resulting solution when the following two solutions are mixed: 50.0 mL of…

A: The given information is: Volume of HNO2 = 50ml = 0.050 L Concentration of HNO2 = 0.500 M Volume of…

Q: Calculate the pH of a solution prepared by dissolving 0.150 mol of acetic acid and 0.300 mol of…

A:

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

A:

Q: Calculate the pH of a 0.10 molar solution of sodium formate

A: Acid dissociation constant of formic acid is:  The chemical equation for the reaction involved with…

Q: What is the pH of a solution that has a [H3O+] = 4.5 × 10^_5?

A: Given:[H3O+] = 4.5 × 10-5 M.

Q: Calculate the percent ionization and the pH of the following solution of phenol, HC6H5O (Ka = 1.3 ×…

A: Given, Concentration of HC6H5O = 2.7 M Ka of HC6H5O = 1.3 × 10-10

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: 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: 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: The pH of a solution with a hydronium ion concentration of 2.17 ´ 10–4 mol/L is       4.34   2.31…

A:

Q: what is the ph of 0.0349 M anilinium hydrochloride (C6H5NH3CI) solution in water, given that K for…

A:

Q: A 0.539 M solution of oxalic acid (pK, = 1.23) is prepared. Determine the pH of the !3! solution.…

A:

Q: Calculate the pH of 0.2 M solution of sodium acetate

A: This is how we can prepare 0.2 M solution. Weigh 27.20 g of Sodium Acetate Trihydrate into a one…

Q: Calculate the pH or the molarity of the following solutions: a) M of a hydronium solution of…

A: (a) • The values provided in the question are:-        i) pH of KOH solution = 11.6    • We need to…

Q: The Kb of hydrazine is 9.1 x 10-7. If 3.12 x 10-3 mol of hydrazine is added to water to make up…

A: Hydrazine (N2H4) is a weak base Concentration of hydrazine is calculated as follows,

Q: Calculate the pH of solutions having the following [H+]: (a) 0.0055 M (b) 1.54 x 10-8 M (c) 3.47…

A: The pH of any solution is given by, => pH = -log[H+ ]

Q: How many moles of (CH3)3N  would need to be added to 459.2 mL of a 0.25 M solution of (CH3)3NHCL  to…

A:

Q: For the reaction of hydrazine (N2H4) in water, H2NNH2(aq) + H2O(l) ⇌ H2NNH3+(aq) + OH- (aq) Kb is…

A: Given: The reaction is as follows: H2NNH2(aq) + H2O(l) ⇌ H2NNH3+(aq) + OH- (aq) The initial…

Q: Acetic acid (CH3COOH, ?a=1.80×10−5) is a weak acid, so the salt sodium acetate (CH3COONa) acts as a…

A:

Q: Calculate the pH of a 0.400 M CH3NH3Cl solution. Kb for methylamine, CH3NH2, is 4.4 × 10-4.

A:

Q: Determine the pH of a 0.24 M solution of sodium acetate (CH3COONa) at 25°C.(Ka of acetic acid = 1.8…

A: Equation for the ionization of CH3COONa is: [CH3COONa] is 0.24 M. It implies 0.24 mols of CH3COONa…

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.