2. What is the pH of 0.0072 M NaOH? 3. What is the pH of 0.00343 M Ba(OH)2? 4. If pOH of a solution is 4.75, what is [OH], [H3O*], and pH?

Q: What is the pH of a 0.310 M solution of HF (Ka = 6.8 × 10⁻⁴)?

A: Recall the expression of pH for weak acid as follows   pH=12pKa-12logC Here HF is a weak acid with…

Q: An unknown weak acid with a concentration of 0.410 M has a pH of 5.600. What is the Ka of the weak…

A: pH is the concentration of hydrogen ion in gram equivalents per litre.it is a measure of acidity or…

Q: solution contains [H+] = 0.0034 M a) What is the pH of the solution?                            pH…

A: Given,  Hydrogen concentration = [H+] = 0.0034 M We need to calculate the pH of the solution using…

Q: What is the [OH] in a solution with a pH of 9.22? (1.7 X 10 M)

A: Given that pH of solution=9.22

Q: A theoretical compound B3(OH)2 is a strong base that has a pH of 13.51. Determine the concentration…

A: The given data is as follows: The pH pf B3OH2 solution = 13.51 The concentration in molarity = ? The…

Q: Determine the [H+] , [OH−] , and pOH of a solution with a pH of 1.03 at 25 °C.

A: Given, pH = 1.03

Q: White vinegar has a pH of 2.4 while apple cider has a pH of about 4.25. What is the difference…

A:

Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.18 M solution…

A:

Q: Solution Y has a pH of 7.5 Solution X has a pH of 9.5   a.) what is the [H3O+] in each solution?…

A: We are given pH and we have to tell H+ and OH- ion concentration

Q: The pH for 0.050 M HNO3?

A: All aqueous solutions always carry particular characteristics in terms of their pH value. [H+] ions…

Q: 6) What is the pH and pOH of a solution with a [OH] of 7.79 X 10* M? Is the solution acidic, basic…

A:

Q: You have a solution with 8.275 x 105 M H3O* a. What is the pH of the solution? b. What is the pOH of…

A: Given: The concentration of H3O+=8.275 x 10-5 M   (a) The pH of the solution can be calculated as:…

Q: 4) What is the [OH] for a solution with a [H,O'] of 9.97 X 104 M? Is the solution acidic, basic or…

A:

Q: (a) What is the pH of 0.65 M potassium formate, HCOOK? (b) What is the pH of 0.85 M NH4Br?

A: An acid is a substance that gives H+ ions in its solution whereas a basic substance gives OH- ions…

Q: What is the pH of a 0.083-M solution of CN−? Use 4.9 × 10−10 as Ka for HCN.

A: To calculate pH of 0.083 M solution of CN-Ka=4.9x10-10CN- +H2O⇌ HCN+OH-So calculate Kb for CN-…

Q: What is the pH of a solution of 0.010 M CH3NH3ClO3?

A: Given that:  [CH3NH3ClO3] = 0.010M CH3NH3ClO3 is salt made up of weak base methyl amine(CH3NH2) and…

Q: What is the pH of a 0.480 M solution of HF (Ka = 6.8 × 10⁻⁴)?

A:

Q: 5. What would the pH of a solution that had a hydroxide ion concentration of 1 x 10º M be?

A:

Q: An aqueous solution has [H+] = 1.0 x 10-4 M. What is the [OH−] for this solution?

A: Given, [H+] = 1 × 10-4 M We have to find [OH-] .

Q: The pH of a 0.152 M solution of a weak acid, HB, is 2.61. What is Ka for the weak acid?

A:

Q: A) What is the concentration of PO43- in a 0.18 M H3PO4 solution?  Ka1= 7.5X10-3 , Ka2=6.2X10-8,…

A: a) The concentration of phosphate ion is calculated as,

Q: The pH of a 2.642M solution of a weak acid, HB is 2.34, What is the Ka for the acid?

A: Given: The conc. of the weak acid solution = 2.642 M HB is a weak acid with a pH = 2.34 A weak acid…

Q: A solution contains [OH-] = 4.88 x 10-6 M. What is the pH of the solution?

A: Given   The concentration of OH- is 4.88×10-6 M.

Q: The molarity of an aqueous solution of NaOH is 0.0022 M. (a) What is the concentration of H3O+ in…

A:

Q: A solution at 25 °C has 3OH-4 = 6.7 * 10-3. What is the pH of the solution?

A: The pOH of a solution is given by, pOH = -log[OH-] The relation between pH and pOH is given by, pH +…

Q: e pH of a 0.125 M solution of HIO3

A:

Q: What is the pH of a solution that is 0.100 M in NaHCO3?

A: Given, 0.100 M in NaHCO3

Q: (a) What is the pH of 0.75 M NaF?(b) What is the pH of 0.88 M pyridinium chloride, C₅H₅NHCl?

A: a) The pH of 0.75 M NaF is 8.52.

Q: What is the pH of 0.0005 M HNO3?

A: The given data is as follows: The concentration of HNO3 = 0.0005 M As we know that HNO3 is a strong…

Q: What is the pH of a solution that has [OH–] of 5.15×10-3 M ?

A: Given, Concentration of hydroxide ion = 5.15×10-3 M

Q: Весause s is a strong acid, it dissociates almost com- pletely in water. That means the…

A: We have given that, the concentration of H+ is nearly equal to the concentration of HNO3.

Q: a) What are [H₃O⁺], [OH⁻], and pOH in a solution with a pH of 3.47? (b) What are [H₃O⁺],…

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

Q: Be sure to answer all parts. What are [H2o), [OH]], and pOH in a solution with a pH of 9.70? [H,O*)…

A: pH = 9.70  [H3O+] = ?  [OH-] = ?  pOH = ?

Q: What

A: Hinderson equation is used for calculating the pH of the buffer solution.  pH = pKa + log( [salt] /…

Q: (a) What is the pH of 0.0333 M HNO₃? Is the solution neu-tral, acidic, or basic? (b) What is the pOH…

A: The pH of any compound can be calculated on the basis of the concentration of hydronium ions present…

Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.58 M solution…

A: Since the Ka1 of H2A is >> Ka2 of H2A  Hence we can assume only the first dissociation of H2A…

Q: (a) What is the pH of 0.65 M potassium formate, HCOOK?(b) What is the pH of 0.85 M NH₄Br?

A: pH is defined as the minus of the logarithm of hydrogen ion concentration([H+]). That is(i.e.),…

Q: What is the pH of 0.0200 M HNO3?

A: Given, 0.0200 M HNO3

Q: You have a solution of HCI with a concentration of 3.258 x 10 10 M. a. What is the {H3O*] of this…

A: Given: Molarity of HCl = 3.258 x 10-10 M

Q: 6) The value of Kw at 37 °C (human body temperature) is 2.1 x 10-14. a) At this temperature what is…

A:

Q: (6)  Is the salt C2H5NH3Cl acidic, basic, or neutral?                            What is the pH of…

A:

Q: The pH of a 2.642 M solution of a weak acid, HB is 5.32. What is Ka for the weak acid?

A:

Q: What is the concentration of H+ in moles/L in a solution that has a pH of 8.35?

A: Given :- pH of solution = 8.35  To calculate :- concentration of H+ ion (mol/L)

Q: pOH

A:

Q: a. What is the pOH of an aqueous solution of 0.483 M hydrochloric acid? pOH =______ b. What is the…

A:

Q: The pH of a 0.224 M solution of a weak acid, HB, is 2.63. What is Ka for the weak acid?

A:

Q: 165 Determine the pH of (a) a 0.40 M CH,COOH solu- tion, (b) a solution that is 0.40 M CH,COOH and…

A: CH3COOH is a weak acid. To calculate the pH, degree of dissociation is calculated first (α) using…

Q: What are [H3O+], [OH−], and pOH in a solution with a pH of 9.90?   [H3O+] = ____×10^__ M   [OH−] =…

A: Given data :

Q: A solution of H2S had a pH of 10.01. What was the [OH-]?

A:

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.