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)

Q: 1. The oxalate ion concentration, C;0. of 0.20 M H;C0 is adjusted to a value of 3.00 x 10 M. What is…

A: As per the guideline, since you have asked multiple questions, we have solved the first question for…

Q: What is the pH of a 0.370 M solution of Ca(NO₂)₂ (Ka of HNO₂ is 4.5 × 10⁻⁴)?

A: Given : Concentration of Ca(NO2)2 = 0.370 M And Ka of HNO2 = 4.5 X 10-4  Since Ca(NO2)2 is a…

Q: What is the pH of a 0.70M KCN solution at 25oC (HCN, Ka=6.17*10-10)

A: Given: 0.70 M KCN solution. Ka of HCN is 6.17*10-10

Q: Calculate the pH of a 0.053 M NaF solution. (Ka for HF = 7.1 x 10−4.)

A: NaF is a salt of strong base (NaOH) and weak acid (HF)

Q: What is the pH of a solution of 0.300 M HNO₂ containing 0.200 M NaNO₂? (Ka of HNO₂ is 4.5 × 10⁻⁴)

A: By using Henderson Hasselbalch equation the pH of the buffer solution is determined by using the…

Q: What is the pH of a 0.860 M solution of Ca(NO2)2 (Ka of HNO2 is 4.5 x 10-4)?

A: A numerical problem based on pH concept, which is to be accomplished.

Q: A 0.432 M solution of pyridine has a pH of 9.40. What is the K, of pyridine? Oa. 2.7 × 104 Ob. 1.5 x…

A:

Q: Q3|| A. Calculate the PH of the (0. 1 N) Na;PO, in 250 ml B. What is the Normality of a sulfuric…

A: The given data contains, concentration of Na3PO4=0.1 N

Q: What is the pH of a 0.01 M CH3COOH solution? (Ka= 1.74 x 10-5)

A: Given that  Ka of Ch3COOH is 1.74× 10^-5    Concentration of Ch3COOH is 0.01M

Q: What is the pH of a 0.390 M solution of HF (Ka = 6.8 × 10⁻⁴)?

A:

Q: What is the pH of a solution of 0.300 M HNO₂ containing 0.110 M NaNO₂? (Ka of HNO₂ is 4.5 × 10⁻⁴)

A:

Q: What are the concentrations of H3O+ and OH− in oranges that have a pH of 3.71?

A: pH :-  The negative logarithm to the base 10 of hydronium ion concentration expressed in mol/L of…

Q: What is the pH of a 0.820 M solution of Ca(NO₂)₂ (Ka of HNO₂ is 4.5 × 10⁻⁴)?

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

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 will be the pH of a solution containing 0.200 M NaH2PO4 and 0.200 M Na2HPO4? Ka(NaH2PO4) = 6.2…

A: Given,  Molar concentration of weak acid, NaH2PO4 or H2PO4- = [H2PO4-] = 0.200 M Molar concentration…

Q: What is the pH of a solution of 0.300 M HNO₂ containing 0.140 M NaNO₂? (Ka of HNO₂ is 4.5 × 10⁻⁴)

A: Given : Concentration of HNO2 = 0.300 M Concentration of NaNO2 = 0.140 M And Ka of HNO2 = 4.5 X 10-4…

Q: Barium fluoride (BaF2) has Ksp = 1.8 x 107. VWhat is the maximum fluoride ion concentration possible…

A: Given: Ksp of BaF2 = 1.8 x 10-7 Concentration of Ba2+ = [Ba2+] = 5.0 x 10-4 M

Q: Calculate the pH of a 0.450 M solution of NH4Cl (Kb for NH3 is 1.8 x 10-5)

A: Interpretation -  To determine the pH of 0.45M of NH4Cl solution when Kb of NH3 = 1.8 ×10-5 .…

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: 2. What is the pH, the pOH and the [OH] of a solution in which the [H*] = 2.43 x 10-6 M? %3!

A: pH is defined as  the negative log of hydrogen ion concentration  pOH is defined as the negative log…

Q: What is the pH of a 0.870 M solution of Ca(NO2)2 (Ka of HNO2 is 4.5 x 10-4)? 1 4 6. 3. LO

A: Data given Ka = 4.5 x10^-4  Concentration of Ca(No2)2 = 0.870 M

Q: Calculate the Ka of a 0.50 M HC4H7O2 with a pH of 2.56

A: The concept used here is based on the acid dissociation constant of an acid which is used for…

Q: What is the pH of a 0.36 M solution of HNO2 (Ka = 4.5 x 10-4)?

A:

Q: What is the pH of a solution of 1.34M nitrous acid( HNO2; Ka=4.0 x10^-4)

A: A numerical problem based on pH calculation, which is to be accomplished.

Q: What is the pH of a solution that is 0.063 M in HA and also 0.023 Min NaA? (Ka = 4.1 × 10- O. 5.46…

A: Given: The concentration of HA is 0.063 M The concentration of NaA is 0.023 M The Ka value is 4.1 x…

Q: 11. What is the pH of 0.25 M NaNO, solution? 2 [Ka of HNO, = 4.0 x 10“] * Points 5.6 6.0 3.7 9.0 8.4

A:

Q: A. Calculate the PH of the (0. 1 N) NasPOa in 250 ml B. What is the Normality of a sulfuric acid…

A: (A) pH of 0.1N Na3PO4 solution: C = 0.1/3 = 0.033M PO43- ions are undergoing hydrolysis and pH is…

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: Find the pH and percent ionization of a 0.200 M HNO2 solution Ka of HNO2= 4.6 x 010-4

A:

Q: What is the pH of a 7.7 x 10-3 M HI solution?

A:

Q: Which of the following is the pH value of the solution containing 0.085 M HNO2 and 0.1 M KNO2? (Ka:…

A: Given, Concentration of HNO2, HNO2 = 0.085 M Concentration of KNO2, KNO2 = 0.1 M Ka = 4.5 X 10-4…

Q: Determine the pH of a 0.0525M Fe(NO3)3 solution.  Ka of Fe3+ = 6.3x10-3

A: Reaction of ferric nitrate in water is given below Fe3+ is formed from Fe(NO3)3.

Q: ) What is the pH of a solution of 0.626 M of a weak base if K, = 3.2x10-³? (Assuming X is very…

A:

Q: What is the pH of a solution with a fluoride concentration of 0.11 M ? The Kb for F– is 1.47×10-11 .

A: The reaction is as follows, The ICE table for above reaction is shown below,

Q: Calculate the pH of a 0.010 M hypochlorous acid solution. For HOCl, Ka = 3.5x10^-8.

A: Given,  The molarity of hypochlorous acid solution is 0.010 M Ka of HOCl is 3.5 × 10-8  The pH of…

Q: What is the pH of a solution of 0.300 M HNO2 containing 0.120 M NaNO2? (Ka of HNO2 is 4.5 × 10¬4)

A: The given data contains, Concentration of weak acid =0.300M Concentration of conjugate base =0.120M…

Q: What are the concentrations of H3O+ and OH− in oranges that have a pH of 3.97?

A:

Q: What is the pH of a solution of 0.300 M HNO₂ containing 0.150 M NaNO₂? (Ka of HNO₂ is 4.5 × 10⁻⁴)

A: In this question, we will calculate the pH of this solution ( this is a buffer solution ). For…

Q: What is the pH of a 0.64 M solution of NH3 (Kb = 1.2 × 10-5)?

A:

Q: Calculate the pH of a solution containing 0.085 M nitrous acid (HNO2, Ka = 4.5 * 10-4) and 0.10 M…

A:

Q: Which of the following is the pH value of the solution containing 0.085 M HNO2 and 0.1 M KNO2? (Ka:…

A: The pH value of the solution containing 0.085 M HNO2 and 0.1 M KNO2, it is to be calculated. Given:…

Q: What is the pH of a solution of 0.300 M HNO₂ containing 0.210 M NaNO₂? (Ka of HNO₂ is 4.5 × 10⁻⁴)

A: BUFFER SOLUTION It is a solution of weak acid or base with their corresponding conjugate base or…

Q: 11. What is the pH of 0.05 M NaNO2 solution? [Ka of HNO2 = 4.0 x 10-4] * O 8.0 O 6.0 O 5.0 O 3.4 9.0

A:

Q: Calculate the pH of 0.0154 M NaN3. (Ka of HN3 = 1.9 x 10-5)

A: NaN3 is a salt of weak acid (HN3) and strong base (NaOH). We know, the pH of salt, which is formed…

Q: What is the pH of a 0.0245 M solution of NH3?        Kb = 1.8 x 10-5

A:

Q: A solution containing two alkaline earth metals ions is made from 0.050 M BaCl2 and 0.025 M CaCl2.…

A: The question is based on the concept of solubility product Principle.   it states that a weak…

Q: Find the pH of a 0.204 M KClO solution. (The Ka of hypochlorous acid, HClO is 2.9×10-8

A: Kclo is a salt of weak acid and strong base so use the formula of PH of salt. PH=10.4

Q: Given the following chemical reaction between a weak acid, HA, and water: НА(аg) Calculate the Ka of…

A: [HA] = 0.546 M  pH = 4.56  We need to determine value of Ka.

Q: Determine the pH of a 0.0525 M Fe(NO3)3 solution. The Ka for Fe3+ is 6.3 x 10^-3. What is the pH?

A: Reaction of ferric nitrate in water is given below Fe3+ is formed from Fe(NO3)3.

Q: What is the pH of a 1.20 M nitrous acid solution? (Ka = 4.50 x 10-4)

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.