What is the pH of a solution when 4.9 g of ammonium bromide, NH,Br (M=98), is used to make 200 ml of solution? NH, (ag) + H;O(I) →H;O•(ag) + NH;(ag) The equilibrium constant Kc= 5.6 x 10-14

Q: Calculate the pH of a 0.381 M NH, solution. NH, has a Kp = 1.8 x 10-.

A: pH: The negative logarithm of H+ ion concentration is known as pH. Ammonia in water behaves as a…

Q: What is the pH of a solution that contains 0.15 M benzoic acid and 0.45 M potassium benzoate? The Ka…

A: Assuming benzoic acid dissolves in water and produces y concentration of ions Since the reaction is…

Q: What is the pH of a solution of 0.300 M HNO2 containing 0.210 M NANO2? (Ka of HNO2 is 4.5 x 10-4)

A: Buffer solution: The solution that resists the change in pH is known as a buffer solution. The…

Q: 11.An acid-base equilibrium system is created by dissolving 0.15 mol HNO2 in water and diluting the…

A: pH change before addition:

Q: The pH of a 0.55 M aqueous solution of hypobromous acid, HBRO, at 25.0 °C is 4.48. What is the value…

A: pH of  HBro = 4.48    -logH+ = pH             H+ =10-pH             H+ = 10-4.48…

Q: Benzoic acid, HC7H5O2, and its salts are used as food preservatives. Ka for benzoic acid is 6,3 x…

A: When an acid undergoes partial dissociation to form protons and conjugate base while a part of the…

Q: What is the pH of a 2.8 M potassium benzoate, KC6H5COO, solution? (benzoic acid Ka = 6.4 * 10-5)

A: The Kb value of benzoate ion is first calculated.

Q: What is the pH of a 0.0650 M solution of methylamine (CH₃NH₂, Kb = 4.4 × 10⁻⁴)?

A:

Q: A sample of potassium acetate, KCH3CO2 (M=98), of mass 4.9 g is used to prepare 500 mL of solution.…

A: Answer: option b. 8.87 is the pH of the solution.

Q: What is the pH of an aqueous solution of 0.159 M sodium cyanide (NaCN)? (Kb of CN- = 2.5 x 10-5)

A: Given, The concentration of sodium cyanide (NaCN) = 0.159 M Kb for CN- = 2.5 x 10-5. pH is the…

Q: 5. The hydronium ion concentration of vinegar is approximately 4 x 10-³M. What are the corresponding…

A:

Q: The PH of 0.0296M HA ( Ka 8.4 *10-9) plus * . . 0.1026 M NaA is 4.3 2 O 8.6 7.5 O

A: The question is based on the concept of PH calculations. we have been given a weak acid and its…

Q: Dimethylamine, (CH3)2NH, a key intermediate in detergent manufacture, has a Kb of 5.9 x 10-4. What…

A: Ionic equilibrium is the equilibrium which is established between the unionized molecules and the…

Q: what is the ph of a 0.85 M solution of pyridine (C5H5N, Kb = 1.70 x 10 ^-9)

A: Pyridine is a weak base. pOH of a weak base. pOH = -log [OH-] pH = 14 - pOH For a weak base like…

Q: Fill in the left side of this equilibrium constant equation for the reaction of carbonic acid…

A: in this question given ka ka= Acid dissociation constant, acid dissociation constant is used to…

Q: What is the pH of a 0.035 M solution of benzoic acid, C6H5COOH? Ką = 6.5 x 10-5

A:

Q: What is the pH of an aqueous solution that is 0.011 M CH3COOH (Ka = 1.8 x 10-5) and 0.019 M…

A: An aqueous solution containing weak acid (CH3COOH) and it's conjugate base (CH3COONa) results in the…

Q: What is the pH of a solution containing 0.30 M NH4OH and 0.52 M NH4Cl? Kb= 1.8 x10-5

A:

Q: Milk of magnesia is a suspension of magnesium hydroxide in water. Although Mg(OH)2 is relatively…

A:

Q: What is the pH of a 0.570 M solution of Ca(NO2)2 (Ka of HNO2 is 4.5 x 10-4)?

A:

Q: If a solution of HF (Ka = 6.8 x 10-4) has a pH of 3.65, calculatethe concentration of hydrofluoric…

A: The term pH of the solution is a measure of the acidity or the basicity of a given solution. More…

Q: The K. of hydrofluoric acid (HF) at 25.0 °C is 6.8 · 10 4 What is the pH of a 0.45 M aqueous…

A: Given Concentration of HF = 0.45 M Ka for HF = 6.8 × 10-4

Q: What is the equilibrium percent ionization of an initially 0.32 M solution of the monoprotic acid…

A: Given that ,  Initial concentration of valeric acid = 0.32 M  Dissociation constant , Ka = 1.44×10-5…

Q: Calculate the pH of a 0.363 M NH, solution. NH, has a Kp 1.8 x 10-5. %3D pH

A:

Q: What is the pH of a 0.690 M solution of Ca(NO₂)₂ (Ka of HNO₂ is 4.5 × 10⁻⁴)?

A: HNO2 ⇌ H+ + NO2- Ka = 4.5x10-4 = [H+][NO2-]/[HNO2] 4.5x10-4 = (x)(x)/0.690 - x  if we assume x is…

Q: What is the pH of a 0.0620 M solution of methylamine (CH,NH2, Kb = 4.4 × 10-4)?

A:

Q: Determine the pH at 25C of a solution prepared by dissolving 0.35 mole of ammonium chloride in 1. L…

A: Concentration of ammonia Volume of ammonia solution  Number of moles of ammonium chloride  added =…

Q: What is the pH of a 0.0580 M solution of hydrocyanic acid, HCN (Ka = 4.9 × 10-1º)?

A:

Q: Hydroxylamine, HONH₂, readily forms salts such as hydroxylamine hydrochloride which are used as…

A: According to the question we have, The concentration of the hydroxylamine (HONH2) is given by (c) =…

Q: 6. What is the pH of a 0.25 M solution of methylamine hydrochloride (CH3NH3CI)? Kb for methyl amine…

A: This ia a salt of weak base and strong acid. So apply formula for salt of weak base and strong acid.

Q: Formic acid is in the venom of some ant species. What is the pH of a 0.35 M solution of formic acid…

A: Given: Concentration of formic acid HA = 0.35 M And Ka of HA = 1.78 × 10-4  The dissociation…

Q: Calculate the pH of a 0.424 M aqueous solution of hydrocyanic acid (HCN, Ka = 4.0×10-10).

A: pH of the solution can be calculated by using the formula,  pH = [H+]. Given data, Concentration of…

Q: Calculate the pH of a 0.100 M NaCH 3CO 2 solution. Ka for acetic acid, CH 3CO 2H, is 1.8 × 103.

A:

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 pH of a solution prepared by dissolving 0.040 moles of sodium nitrite (NaNO2) in 200…

A: When HNO2 and NaNO2 are mixed, they form buffer solution HNO2/NO2-. And the pH of a solution is…

Q: What is the pH of 0.273 M trimethylammonium iodide, (CH3)3NHI? The Kb of trimethylamine, (CH3)3N, is…

A: Kb = 6.3 x 10-5

Q: 1) Calculate the pH of a solution prepared by dissolving 1.15 g of sodium acetate, CH3COONa, in 71.0…

A: Find the moles of Sodium Acetate  find the moles of Acetic acid  then find the ph using henderson…

Q: Calculate the pH and the concentrations of all the species present in 0.010 M of Carbonic acid…

A:

Q: Alizarin yellow R, Ka = 7.9 x 1012, is yellow in its protonated form (HX) and red in its ionized…

A: Alizarin yellow (R)  be a distinct orange color when,…

Q: When 0.040 mol of propionic acid, C2H5CO2H, is dissolved in 700 mL of water, the equilibrium…

A: Molarity is solution expressed as the number of moles of solute per litre of solution. Equilibrium…

Q: 2. Calculate the pH of a solution containing 0.75 M lactic acid, HC3H5O3, (Keq= 1.4 x 104) and 0.25M…

A: The solution contains a mixture of 0.75 M lactic acid and 0.25 M sodium lactate.

Q: Consider two aqueous solutions of equal concentration: chlorous acid (HCNO, K, 2.0 x 10 4) and…

A: The dissociation constant Ka is used for the quantitative measurement of the strength of the acid.…

Q: What is the pH of a 0.1055 M CH3COOH solution (K, = 1.75 x 10-5)? %3D

A: Answer: ICE table for the dissociation of weak monoprotic acid is shown below:

Q: The Ka of hypobromous acid, HOBr, is 2.6 x 10-9. Calculate the pH of a solu tion which is composed…

A: PH of acidic buffer can be calculated as follows

Q: What is the pH of a 1.00 x 10^-9 molar solution of KCl?

A: KCl is a salt of strong acid (HCl) and strong base (KOH).

Q: What is the pH of a 0.0680 M solution of hydrocyanic acid, HCN (Ка %3D 4.9 х 10-10)?

A:

Q: HCIO is a weak acid (K. = 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…

A:

Q: What is the concentration of calcium ion, Ca2+ (in x 10-3 M) in a solution of calcium hydroxide,…

A:

Q: Calculate the pH of a 42mL solution containing 3.7g of hydrofluoric acid.  Ka = 6.6 x 10-4

A: Given: Ka for hydrofluoric acid = 6.6 x 10-4 We have to calculate the pH of a 42 mL solution…

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.