What is the pH of a 0.250 M HOCI solution? K, of HOCI at 25°C is 3.5 x 10-8. O 7.46 O 4.03 O 3.57 O 9.97

Q: What is the pH of a 0.0257 M solution of NaOH (γγOH- = 0.889)?

A:

Q: The Kb of C6H5NH3+ is 3.98x10-10 What is its Ka? What is the [H3O+] concentration in a solution…

A:

Q: Calculate the pH of a solution that is 0.0729 M LiC2H3O2 at 25°C.

A: LiC2H3O2 ( Lithium acetate) is the salt of a weak acid and strong base.   LiC2H3O2 → CH3COO- +…

Q: A solution of 0.00100 M HCI has a pH of: (HCl is a strong acid and dissociates completely in…

A: Given that, Concentration of HCl acid = 0.00100 M Since, HCl is a strong acid, it completely ionised…

Q: What is the pH of a 0.0520 M solution of HONH,CI (Kb of HONH, is 1.1 × 10*)? 2

A: Solution :      Weak bases show partial ionization on dissociation in an aqueous solution. Here…

Q: A solution has a pOH of 6.50 at 50∘C. What is the pH of the solution given that Kw=6.22×10−15 at…

A: To determine pH of solution: First we have to calculate pKw,

Q: CH3NH2 is a weak base (?b=5.0×10^−4), so the salt CH3NH3NO3 acts as a weak acid. What is the pH of a…

A: CH3NH3NO3 → NO3- + CH3NH3+ Kb for the above reaction is 5x10-4  CH3NH3 can donate a proton and…

Q: The pH of a basic solution is 12.35. What is [OH 1?

A: pH + pOH = 14  Given, pH = 12.35  Then , pOH = 14-12.35 = 1.65

Q: What is the pH of a 0.0352M solution of NaOH?

A: pH = - log [H3O+ ] pOH  = - log [OH-] pH + pOH  = 14

Q: em101 The pH of a 0.0049 M solution of Ca(OH), is

A: Given that: molarity of Ca(OH)2 = 0.0049 M To find: pH of 0.0049 M Ca(OH)2 solution?

Q: What is the pH of a 0.2 M HNO2 solution if percent ionization is 1.2%?

A: PH = - log(H+) Percentage of ionisation = 1.2 HNO2 are in 0.2M

Q: what is the pH of a 3.25x10^-4M solution of H+?

A:

Q: What is the pH of a solution with a hydrogen concentration of 8.6x10-2M?|

A:

Q: The pH of a Solution is 1.411. what is the p OH? what is the [H30 ]? what is the TOM]?

A:

Q: W

A:

Q: A pH of an aqueous solution at 25 C is 8.80. What is the [OH-] concentration in this solution? Kw =…

A: pH :- It is defined as the negative logarithm to the base 10 of hydrogen ion concentration expressed…

Q: A sample of fruit juice is found to have à hydrogen concentration of 2.87 x 104. What would the pH…

A: Given hydrogen ion concentration of fruit juice is 2.87*10-4. We have to determine PH of fruit…

Q: . What is [OH⁻]?

A: The pH of a solution is determined as the negative logarithm of the concentration of hydrogen ions…

Q: The pH of a basic solution is 10.41. What is [OH⁻]?

A: pH of a solution is the parameter which is used to define the acidity or basicity of a solution.…

Q: what is the pH of a 0.140 M solution of NH4Cl? ka for ammonium is 5.68x10^-5

A: A salt that contains either weak acid ions or weak base ions does not exact 7 pH values. Its pH…

Q: Calculate the pH of HOCI solution that is 2xE-6 M, Ka =2.8xE-8 а. 2.8 O b. 2.4 O c. 1.3 O d. 6.6

A:

Q: Calculate the pH of an aqueous solution at 25°C that is 0.29M in phenol (C,H;OH ). (K, for phenol =…

A:

Q: Q49 (Ex. 13.6) In chemistry, the pH value . measure.. acidity. The pH value is defined by pH where…

A: pH :-  It is defined as the negative logarithm to the base 10 of hydrogen ion (H+ ion )…

Q: Novocaine, C13H21O2N2Cl, is the salt of the base procaine and hydrochloric acid.  The Kb of procaine…

A: Salts are of three types .They are Acidic salt , basic salt and neutral salt.

Q: The concentration of H* (or H3O*) from part A should be 1.02x×10-2 mol L-1. What is the pH of the…

A:

Q: What is the pH of IxE-9 M HCI solution? O a. 6.99 O b. 9.00 Oc. 9.1 O d. 7.5

A: Answer: option b. 9.00 is the pH of the HCl solution.

Q: The pain reliever codeine is a weak base with a K, equal to 1.6x10-6. What is the pH of a 0.05 M…

A: pH of a solution is defined as the negative  logarithm of H+ ion concentration. Given codeine…

Q: If a sample of a certain solution is determined to have a [H3o+ ]concentration of 9.25×10 -4…

A:

Q: pH of a 10-4 M KOH solution is: O -4 O 10 O 4 O -10

A: pH is the negative logarithm of the concentration of Hydrogen ion and is given by  pH = - log [H+]…

Q: Hydrazine, N2H4, has Kb = 1.3E-6. Calculate the pH of a 0.644 M solution of N2H4.

A:

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

A:

Q: The pH of a solution is 6.88. Find the H + and OH- concentrations and pOH

A: pH is a scale used to determine the H+ ion concentration of a solution. pH is numerically negative…

Q: Determine the pH of each of the following solutions: a. 0.125M NH,CI (aq), K, for NH3 = 1.8x105 b.…

A:

Q: What is the pH of a solution that has a hydrogen ion con- centration of 1.0 X 10 M? 46. TATI

A:

Q: A solution has a pOH of 7.1 at 10∘C. What is the pH of the solution given that Kw=2.93×10−15 at this…

A: Kw=2.93 x10-15pkw=-log 2.93x10-15     =15-log 2.93pkw=15-0.466=14.534pH+pOH=pkwpH=pkw-pOH…

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: Calculate the pH of the following solutions.  1.50 g of NaOH in 50 mL of the aqueous solution

A: Given: The amount of sodium hydroxide present in 50 mL of water is 1.50 g.

Q: 3. The [OH] of a solution is 5x10(-6) M. What is the pH? O 6.7 8.3 8.7 6.3

A: First of all, we will calculate the concentration of [H+] from ionic product of water and from there…

Q: What is the pH of a solution with hydroxide concentration, [OH--] = 4.83×10-5 M?

A: According to the question,  We need to calculate the pH of a solution with hydroxide concentration,…

Q: The pH of an aqueous solution at 25oC is 2.40. What is the [OH-] concentration in this solution? Kw…

A: Given data :- pH = 2.40 Temperature = 25℃ Kw = 1.0 × 10-14 We know that ., PH + POH  = 14

Q: If the [OH] of and acid is 2.57 x 10-8, what is the pH? o 13.2 o 12.49 ○ 6.41 o 2.91

A:

Q: A solution of sodium acetate 1NaCH3COO2 has a pH of 9.70. What is the molarity of the solution?

A: pH scale is used to measure the acidity or basicity of the solution. If the solution is acidic in…

Q: Hydrazine, N2H4 has Kb= 1.3E-6. Calculate the pH of 0.486M solution of N2H4.

A: Hydrazine is a weak base.We have to calculate pH given hydrazine solution. Recall the following…

Q: What is the pH of the following solution? 3.9*10^-5 M H3O- at 25 degrees Celsius  A) 5.41 B) 8.59…

A:

Q: f 0.30 M of ammonia solution has a pH of 9.11, what is the H+ concentration of the solution?

A: Given pH = 9.11

Q: 300.0 mL of a 0.385 M solution of NaI is diluted to 700.0 mL. What is the new concentration of the…

A: Given,  300.0 mL of a 0.385 M solution of NaI is diluted to 700.0 mL. The new concentration of the…

Q: Potassium hydroxide is classified as a base because KOH contains O a K* ions O b 0²- ions OH- ions O…

A: Given here potassium hydroxide is classified as a  base.we are asked to choose option in the given.

Q: A solution with (OH- )of 5 x 10^3 has a pH of? A.-2.3.   B. 11.7.   C 7.0. D. 2.3

A: (b) 11.7 Concentration of OH- ions = 5×10-3 Now, pOH = -log[OH-]                    = -log (5×10-3)…

Q: The PH of a solution containing a [H3O+]= 3.40 x 10 -5 M, is: a. 1.67 b. 3.40 c. 4.47 d. 12.3

A: Given : [H3O+ ] = 3.40 X 10-5 M

Q: If the pH of a solution is 6, then O [OH--] = 1 x 10 8 M O [H+] = 6 M O [H+] = 1x 106M O pOH = 1

A: Given that pH of a solution is 6.We know pH = - log [H+].Thus we can get the [H+] as 10^…

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.