Calculate the pH of 0.050 M NaClO if Ka for HClO is 3.5E-8.

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

A: Ka of HClO is given as 4 x 10-8. It is required to calculate the pH of solution that is 0.054M in…

Q: 3. Calculate the pH of a 0.600M solution of Na2S

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Q: Calculate the pH of a 0.0095 M solution of acetic acid, HCH3CO2,  Given Ka= 1.76x10^-5

A: Acetic acid is a weak acid so it will dissociate very less in the solution. First of all a balanced…

Q: Calculate the pH of a 0.10 M HCOOH solution. Ka of HCOOH is 1.8 X 10-4.

A: pH is defined as the negative logarithm of hydrogen ion concentration present in the solution.…

Q: Calculate the pH of a 0.043 M NaF solution. (K, for HF = 7.1 x 104.)

A: Given -> Molarity of NaF = 0.043 M Ka ( HF) = 7.1 × 10^ -4

Q: The pH of a 0.15-M solution of HSO4− is 1.43. Determine Ka for HSO4− from these data.

A: Given, initial concentration of HSO4− = 0.15 M            pH = 1.43 We know that, pH is the negative…

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

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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: What is the pH of a 0.0520 M solution of HONH;CI (Kb of HONH2 is 1.1 x 10-8)?

A: HONH3Cl is a salt of weak base HONH2 and strong acid HCl Recall the following expression to…

Q: What is the pH of a 0.720 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

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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 .10 M solution of formic acid (HCHO2). The Ka of formic acid is 1.8 x 10-4.

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Q: 7. The pH of a 0.10 M solution of acetic acid (CH3COOH) is 2.39. What is the Ka of acetic acid?

A: H3O+ can be calculated as follows: pH=-log [H3O]+[H3O]+=10-pH[H3O]+=10-2.39[H3O]+=0.00407 M

Q: What is the pH of a 0.650 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

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Q: Calculate the pH of a 3.12×10-3 M  solution of NaF, given that the Ka of HF = 6.80 x 10-4 at 25°C.

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Q: Calculate the pH of a 0.350M aqueous solution of NH3 , The Kb of NH3 is 1.77 x 10-5

A: Given: The concentration of aqueous NH3=0.350M

Q: Using data from Appendix D, calculate 3OH-4 and pH for each of the following solutions: (a) 0.10 M…

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Q: What is the pH of a 0.1966 M HCOOK? Ka for HCOOH is 1.74e-4.

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Q: If the pH of a 0.0850 M solution of HB1O2 is 2.29, then what is the value for the acidity constant,…

A: HBrO2 +     H2O →     H3O+   +    BrO2-Initial              0.0850…

Q: Calculate the pH of a 3.97×10³ M solution of NaF, given that the Ka of HF = 6.80 x 10-4 at 25°C.

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Q: Determine the pH of each of the following solutions. (a) 0.684 M hypochlorous acid (weak acid…

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Q: Calculate the pH of 2.5 M CH2ClCOOH(aq) given that its Ka = 0.0014.

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Q: The pH of a 0.0492 M solution of a weak acid is 2.641. What is the Ka of the acid?

A: pH= 2.641

Q: The pH of a 0.02 M NgOH solution at 25 °C is: O 12.8 O 13.7 O 1 1.5 O 12.3 O 13.1

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

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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: For HNO2, Ka = 4.6 x 10-4 and for HSO4-, Ka = 1.2 x 10-2. Which is the stronger acid?

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Q: The pH of a 0.23-M solution of HF is 1.92. Determine Ka for HF from these data

A: The pH of a solution is used to determine the acidity or alkalinity of a solution. The pH is given…

Q: Calculate the percent ionization in a 0.040 M NH3 solution, given that the pH of the solution is…

A: The concentration of the NH3 solution is = 0.040 M The pH of the solution is = 11.50 The percent…

Q: The pH of a solution at 25°C in which [OH]= 2.0 x 10 is: 1 9.52 4.76 4.69 3.30 9.30

A: In this question, we want to determine the pH of the Solution.  You can see details Solution below…

Q: Calculate the pH of a 0.31 M sodium formate solution (HCOONa).   Kb for HCOO− = 5.9 × 10−11

A: Given :-  [HCOONa] = 0.31 M  Kb for HCOO- = 5.9 × 10−11  To calculate :-  pH of solution

Q: Calculate the pH of a 0.20 mol L 1 solution of boric acid (H3 BO3) at 25°C. The value of K, for the…

A: Equilibrium is defined as the state at which the rate of forward reaction becomes equal to the rate…

Q: 1. Calculate the pH of a 0.045M sulfurous acid solution. H,SO, → H* + HSO, Ка, = 1.7 x 102 HSO3- H +…

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Q: The pH for a solution with a [H3O]+ of 1.0 x 10^-6 is

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

A: It is required to calculate the pH of the solution that is 0.016 M in NaClO.Ka for HClO = 4 x 10-8…

Q: The pH of a 0.05 M NaOH solution at 25 °C is: O 13.8 O 13.1 O 1.5 • 12.7 O 10.3

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Q: Determine the pH level

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Q: Calculate the pH of a 0.10 M solution of sodium acetate (NaCH3COO) given that the Ka of acetic acid…

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Q: Calculate the pH of a of 0.100M KBRO solution. Ka for hypobromous acid, HBRO, is 2.0 x 10 6- 10.85…

A: Given: The concentration of the KBrO3 solution = 0.100 M The Ka for HBrO3 = 2.0 × 10-9 We have to…

Q: 5. Calculate the pH of a 0.00339 M solution of NaF. (K, for HF is 6.6 x 104).

A: This question is related to finding the pH of given solution. First find out the components of it.…

Q: Calculate the pH of a solution with [H,O*] of 8.96×10 4 pH =

A:

Q: In an aqueous solution at 25°C, if [H₃O⁺] = 1.1 × 10⁻⁴ M, then [OH⁻] is:

A: We know that  Kw  for water  =  10-14 at 25oC Given [H3O+] concentration is 1.1×10-4 M      [ OH-] =…

Q: What is the pH of a solution with [H3O+] of 1.9 x 10-8 M?

A: Given that, [H3O+] = 1.9×10-8 M pH = ?

Q: Calculate the pH of a 1.60 M KBRO solution. Ka for hypobromous acid, HBrO, is 2.0 × 10º. 4.25 2.55…

A: ph is the gives the hydrogen ion concentration in the aqueous solution.

Q: Calculate the pH of each of the following solutions (Ka and Kb values are given in Appendix D) 0.100…

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Q: Determine the pH of a solution that is 0.00542 M HCl and 0.0513 M HClO2. The Ka of HClO2 is 1.1 ×…

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Q: What is the pH of a 0.420 M solution of C5H,NHB (Kb of C5H,N is 1.7 × 10-9)?

A: Given:: [C5H5NHBr]=0.420 M =concentration of salt=c Kb of C5H5N = 1.7×10-9 pH=?

Q: Determine the pOH of a 0.461 M C,H5 COOH solution if the Ka of the acid is 6.5 X 10-5 5.48 O 11.74…

A: We will first write dissociation equation of acid, then calculate H+ concentration to find pH and…

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: An acid is a substance that can furnish the hydrogen ions in the aqueous solution. The weak acid…

Q: Calculate the pH of water containing 0.05 M NaCl at 25°C. Given: YH = 0.86 and %3D YOH- = 0.81. O…

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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.