6. How many moles of benzoic acid (HC-HsO2) must be used to prepare 500. mL of a solution that has a pH of 2.44? Note that the Ka of benzoic acid is 6.3 x 10°.

Q: What is the pH of a 0.400M solution of sodium acetate?

A: The chemical formula of sodium acetate is CH3COONa. It is a salt of strong base NaOH and weak acid…

Q: How many moles of NO3 - are present in 250.0 mL of a nitric acid solution having a pH of 5.10?

A: Nitric acid is strong acid , having dissociation constant equal to 1. pH of any substance is…

Q: Phenylacetic acid (C6H5CH2COOH, simplified here to HPAc; see model) builds up in the blood of…

A: Solution- Given data: The pH of Phenylacetic acid = 2.62. The concentration of C6H5CH2COOH…

Q: The Ka, for propionic acid, HC3H5O2, is 1.30 x 10^ -5. What is the pH of a 0.0850 M propionic acid…

A: The dissociation reaction of propanoic acid is given by  HC3H5O2 -----> H+ + C3H5O2- hence Ka = […

Q: Phenylacetic acid (C6H5CH2COOH, simplified here to HPAc) builds up in the blood of persons with…

A: Given data: The pH of Phenylacetic acid = 2.62. The concentration of C6H5CH2COOH [C6H5CH2COOH] =…

Q: What is the pH of a solution that is 2.0 M HF and 2.0 M F–?  Does your answer make sense?

A: The Henderson Hasselbalch equation for acidic buffer is given as :

Q: what is the ph of a solution that is 0.100 m in hydrofluoric acid? The Ka of hydrofluoric acid is…

A: Recall the following expression to find pH of the given solution of hydrofluoric acid. Given that…

Q: 1. Given that methylamine, CH3NH2, has a Kb of 4.4 x 10-4, what is the pH of a 0.20 M aqueous…

A: Given : Kb = 4.4 × 10-4 Concentration of methylamine = 0.20 M

Q: 4. A 0.020 M weak acid HA, has a pH of 3.21. What is the Ka of the acid?

A:

Q: What is the acid-ionization constant, Ka, for this acid?

A: Given data contains, Concentration of HA is 0.200 M. pH is 2.210. The given chemical equation is,…

Q: A 0.107 M solution of Providenol, a weak acid, has a measured pH of 4.32. Determine the pKa of…

A: The equilibrium constant depicting dissolution of either weak acids/base is known as dissociation…

Q: HCN is a weak acid (Ka=6.20×10−10), so the salt, KCN , acts as a weak base. What is the pH of a…

A: Ka = 6.20×10-10 pKa = -log(Ka)    = -log(6.2×10-10 = 9.21  Concentration(C) of salt =0.0750 M

Q: Phosphoric acid, H3PO4 is a triprotic acid. pKaj= 2.16 pКа237.21 pКаз-12.32 2- Calculate the pH of a…

A: Phosphoric acid will ionize in aqueous solution as--

Q: What is the pH of a solution that is 0.15 M NH4Cl and 0.35 M NH3?   The Ka of NH4Cl is 5.01 x…

A: In this question , we have to calculate the correct pH of given problem by the help of…

Q: The Ka of hypobromous acid, HOBr, is 2.6x10-9. Calculate the pH of a solution which is composed of…

A: Given :-  [HOBr] = 0.40 M  [NaOBr] = 0.40 M Ka for HOBr = 2.6 × 10-9  To calculate :-  pH of…

Q: Methylamine, CH3NH2, has a Kb = 4.40 x 10-4. What is the pH of a 0.450 M  solution of methylamine?

A: Methylamine, CH3NH2 is a weak base which undergoes partial dissociation in aqueous medium. Let the…

Q: What is the pH of an aqueous solution in which [H+] is 0.0025 M?

A:

Q: HA(aq) is a weak acid with a dissociation constant, Ka, of 8.8 x 10−12. What is the pH of a 0.022 M…

A:

Q: Calculate the pH of the following aqueous solution:           0.40 M NH 4Cl (p K b for NH 3 = 4.74)

A:

Q: What is the pH of a 0.16 M solution of methylammonium chloride, CH;NH; Cl? What is the concentration…

A:

Q: How many moles of NH3 must be dissolved in water to give 813.0 mL of solution with a pH of 11.15? Kb…

A: The value of Kb for the given weak base is = 1.8x10-5 The concentration of the base solution is =?…

Q: HClO is a weak acid (?a=4.0×10^−8) and so the salt NaClO acts as a weak base. What is the pH of a…

A: Given : Concentration of NaClO = 0.014 M Since NaClO is a weak conjugate base of weak acid HClO.…

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

A:

Q: Calculate [H+ ], [OH- ], pH and pOH of: a) 2.00 M (weak acid) HF  (Ka=6.8 x 10 -4) b) 0.1 M HNO3

A: a) concentration of HF = 2.00 M  Ka = 6.8 × 10-4  [H+], [OH-] , pH &  pOH = ?  b) concentration…

Q: Consider the weak acids, HCN and H 2CO 3. a. Which acid has the larger Ka? b. Which acid is…

A: Since you have posted multiple sub-parts, the answer for first three sub-parts are given below.…

Q: What is the pH of a solution made by adding 0.50 mol of formic acid (HCOOH) and 0.50 mol of sodium…

A: Given: Number of moles of formic acid= 0.5 mol Number of moles of sodium formate = 0.5 mol To find:…

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: What is the pH of a 8.1 × 10-6 M KOH solution?

A: The pH scale is introduced by the scientist Sorensen in order to express the [H3O+] ion of a…

Q: If the ph of 0.10 M HA (weak acid) is 4.10, calculate Ka for this weak acid.

A: From given pH value the hydronium ion concentration is determined first.

Q: A beaker holds a mixture of 0.40 M HIO3 and 1.0 M HCOOH. Ka(HIO3) = 1.6 x 10-1 Ка(нсоон) = 1.77 ×…

A: Given: Ka (HIO3) = 1.6 × 10-1 Ka (HCOOH) = 1.77 × 10-4 We have to calculate the pH of a mixture of…

Q: 1. Calculate the pH of a solution prepared by dissolving 2.13 g of picric acid, (NO2);C6H2OH (229.11…

A:

Q: When 0.100 moles of NaX salt are dissolved in water to a volume of 1.00L, the pH and solution is…

A:

Q: What is the pH (in two decimal places) of a 0.047 M solution of Sr(OH)2?

A:

Q: Methylamine, CH3NH2, has a Kb = 4.40 x 10-4.  What is the pH of a 0.290 M  solution of methylamine?

A:

Q: The pH of a 0.5 M aqueous solution of formic acid, HCHO2, at 25.0 °C is 2.0. What is the value of Ka…

A: pH tells us about the acidic or alkaline values of a solution. Dissociation of a weak acid depends…

Q: The acid dissociation constant K of boric acid (HBO3) is 5.8 × 10¯¹0. Calculate the pH of a 2.5 M…

A:

Q: What is the pH of 0.25 M ethanolamine?

A: To calculate the pH of 0.25 M ethanolamine

Q: The pH of a 0.50 M aqueous solution of a weak acid at 25.0 °C is 1.43. What is the value of Ka for…

A:

Q: Enough water is added to 0.35g of benzoic acid to make 1000 mL of a solution. What is the pH?…

A: Given: Mass of benzoic acid=0.35 g Volume of solution=1000 mL =1 L Ionization constant for benzoic…

Q: What is the pH of a solution that is 0.041 M in NH4Cl?

A: NH4Cl salt can be formed from weak base NH4OH and strong acid HCl. So it is a salt of strong acid…

Q: What is the concentration of hydroxide ion in a 0.150 M aqueous solution of hydroxylamine, NH,OH?…

A: NH4OH is a weak base, hence it can't dissociate completely, hence equilibrium is established between…

Q: Calculate the pH of a solution prepared from 3.0 g of acetic acid to 500 mL of water.

A: Solution: pH is the measure of hydrogen ion strength of a solution and its value is equal to the…

Q: If a weak acid  (HA) has a Ka of 1.35 x 10-8, what is Kb for A-, the conjugate base.

A: If a weak acid (HA) has a Ka of 1.35 x 10-8, the Kb for A-, the conjugate base is to be calculated.

Q: What is the concentration of a formic acid (HCHO,) solution with a pH = 3.15? The K, of formic acid…

A: given :- pH of solution = 3.15                Ka of formic acid = 1.8 × 10-4 to calculate :-…

Q: What is the pH of a solution prepared by dissolving 1.2 g of Ca(OH)2 in water to make 925 mL of…

A: First, calculate the molarity of calcium hydroxide,

Q: 3. Designate the Lewis acid and Lewis base in each of the following reactions: ÇI CH, CH,-C-OH, ČH,…

A: Anything that occupies space and has mass is called matter. The matter may be classified into acids…

Q: The Ka for HC2H3O2 is 1.8 x 10-5. What is the pH of a 0.02M solution of this weak acid?

A:

Q: If 7.4 g of butanoic acid, C, H, O,, is dissolved in enough water to make 1.0L of solution, what is…

A: Mass of butanoic acid =7.4 g Molar mass = 88g/mol Moles = 7.4g/88g/mol= 0.0841 moles Volume of…

Q: 1. Which has the lowest pH? Explain why. 0.10M HCl or 0.20M HCl

A:

Q: What is the pH of a 4.9 × 10-6 M KOH solution?

A: given :- concentration of KOH solution = 4.9 × 10-6 M  to calculate :- pH of solution

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.