Calculate the [OH−] of a solution of 0.1595 M C5H5NH3F if Kb = 1.800e-9 for C5H5NH2?

Q: 9. A solution with a pOH of 4.65 at 25°C has a pH of .

A:

Q: 5) What are the [H3O*] and pH of 0.085M weak base C2H5NH2?

A: The question is based on the concept of chemical equilibrium. we have to calculate PH and hydronium…

Q: What is the pH of a 0.65M NaClO solution. (Kb=3.448x10^-7)

A: Negative Logarithm of concentration of [H]+present in the solution is known as pH of the solution.

Q: For a 0.0037 M solution of HCIO4, the dissociation of water produces the following concentrations of…

A: HClO4 is a strong acid, so, it undergoes complete ionization in the aqueous solution. HClO4 -->…

Q: Calculate the pH of a 1.16 M aqueous solution of pyridine hydrochloride (C5H5NHCl). (For pyridine,…

A: Given :

Q: For H3PO3, Ka1= 4.06x10^-2 and Ka2= 3.92x10^-7. Calculate the pH of 0.295 molar solution H3PO3

A:

Q: Determine the pH of a 0.35 M aqueous solution of CH3NH2 (methylamine). The Kb of methylamine is 4.4…

A: Given- Concentration of CH3NH2 = 0.35 M Kb = 4.4 × 10-4 To find - pH of solution Formula- pH = - log…

Q: Calculate the [H3O+] of a solution of 0.1769 M LiOCl if Ka = 3.500e-8 for HOCl?

A:

Q: culate the [OH-]of the solution with pH=10.50 3.2 x 10-10 1.05 x 10-10

A: pH is defined as negative logarithm of hydrogen ions present in solution.

Q: What is the pH of a solution that is 0.21 M CH3NH2 (methylamine) and 0.31 M CH3NH3Cl (methylammonium…

A: Since CH3NH2 is a weak base with pKb = 3.38 And the solution is having CH3NH2 and its conjugate acid…

Q: For a 0.0494 M aqueous solution of cyanic acid, HCNO (Ka = 3.5*10-4), determine the following. What…

A: Given Data : 1. Molarity of cyanic acid solution = 0.0490M 2. Dissociation constant of cyanic acid…

Q: Determine the pH of a 0.22M NaF solution at 25 degrees Celsius. The Ka of HF is 3.5 x 10-5

A: We have to calculate the pH of 0.22 M NaF solution.

Q: Aspirin is acetylsalicylic acid, HC,H,O4, which has a K, of 3.0 × 10¬4. Calculate the pH of a…

A: Given information: Mass of acetylsalicylic acid = 0.65 g Volume = 50.0 mL

Q: Calculate the pOH in 0.3582 M H3PO4. The stepwise dissociation constants are Ka1 = 7.50e-3 and Ka2 =…

A:

Q: A solution of 0.05 M in NH4CI and 0.03M in NH3, calculate its OH- concentration and its pH. (pKa…

A: Concentration of NH4+ = [NH4+] = 0.05 M Concentration of NH3 = [NH3] = 0.03 M OH- concentration of…

Q: Calculate the OH- for a 0.300 M solution of pyridine, Kb = 1.7 x 10^-9

A:

Q: What is the pH of a 0.1250 M CH3NH3Br? Kb for CH3NH2 is 3.70e-4.

A: Given,  The pH of a 0.1250 M CH3NH3Br is : Kb for CH3NH2 is 3.70e-4.

Q: Calculate the hydronium and hydroxide ion concentration at 25°C in a. 0.15 M H2SO4 b. 8.4 × 10−3 M…

A: For aqueous solution, the product of the concentration of hydronium and hydroxide ions is given by:

Q: Calculate the [OH −] of a solution of 0.1134 M CH 3CH 2NH 3Cl if K b = 6.400e-4 for CH 3CH 2NH 2?

A:

Q: Calculate the pH of a solution with [OH]] of 6.58×106. pH = %3D

A:

Q: Calculate the equilibrium concentration of the nonionized bases and all ions in a solution that is…

A:

Q: What is the pH of a solution that is 0.125 M in maleic acid, a DIPROTIC acid with Ka1=1.2x10-2 and…

A: Maleic acid dissociates in two steps. The major concentration of hydrogen ion is released in the…

Q: 5) What are the [H3O+]and pH of 0.085M weak base C2H5NH2?

A: Concentration of C2H5NH2=0.085M [H3O^+]=? pH=?

Q: Calculate the pOH of an aqueous solution at 25°C that is (a) 0.011 M in HNO3 , (b) 3.5 × 10-3 M in…

A: pOH of solution can be can be calculated as, pH=-log[H+]pH+pOH=14pOH=14-pH

Q: Calculate [H3O + ] and [CH3COO− ] in an aqueous solution that is 0.100 M in both CH3COOH and…

A: Introduction: pH: pH is used to express the acidity of the solution. It is defined as the negative…

Q: Calculate the pH of an aqueous solution at 25°C that is (a) 0.035 M in HI, (b) 1.2 × 10-4 M in HNO3…

A: pH can be calculated by using the formula, pH=-log(H+)

Q: The Kb of dimethylamine [(CH3)2NH] is 5.90×10-4 at 25°C. Calculate the pH of a 1.10×10-3 M  solution…

A:

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: Calculate the pH of a solution prepared by dissolving 3.90 g of sodium acetate (NAC2H3 of solution.…

A:

Q: Calculate the pH of 0.750 M pyridinium chloride, C5H5NHCl? Given Kb of C5H5N is 1.70×10-9.

A:

Q: What is the pOH of a 0.1563 M NH4NO3? Kb for NH3 is 1.86e-5.

A: Given: kb for NH3 = 1.86 * 10-5 concentration of NH4NO3 =  0.1563 M

Q: Calculate the pH of a 0.20 M H2A solution that has the stepwise dissociation constants Ka1 = 1.5 ×…

A: To find pH.

Q: What is the pH of a solution that is 0.26 M CH3NH2 (methylamine) and 0.38 M CH3NH3Cl (methylammonium…

A: The basic buffer may be explained as the solution mixture which hold the weak base along with its…

Q: The pH of a solution at 25C 11 which OH =20x 10 is: 4.76 3.30 9.52 9.30 4.69

A: Concentration of OH- ion = 2.0 × 10-5  pH of the solution at 25°C = ?

Q: Calculate the [OH] in 0.2110 M H3PO4. The stepwise dissociation constants are Ka1 = 7.50e-3 and Ka2…

A:

Q: %3D What is the pH of a 0.1000 M NACH3COO solution? (Ka CH3COOH = 1.8x10^-5) 4.75 5.13 8.87 7.45…

A: We have find out pH of 0.1000 MNaCH3COO Solution.

Q: What is the pH of a solution with H30+ =4.5 × 10^-5  M? 5.4 6.2 11.0 4.3

A:

Q: Calculate the pH of a solution containing 0.20 M HN3 and 0.30 NH4Cl, Kb=1.8x10-5

A: pOH of a solution containing salt and base can be calculated by using the equation :…

Q: Determine the pH and the type of solution of a 0.227 g/L C5H5N solution at 25°C.  The Kb of C5H5N is…

A: At 25°C Concentration=0.227g/L Kb of C5H5N = 1.7 ×10^-9

Q: What is the approximate pH of a solution formed by mixing 45.0 mL of 0.10M HNO3, 50.0 mL of 0.20M…

A: Given: The volume of HNO3=45.0 mL  Molarity of HNO3=0.10M  Volume of HCl=50.0 mL  Molarity of…

Q: In the following equation HNO2 (aq) + H2O (l) ↔ H3O+ (aq) + NO2-(aq), 0.37 M of nitrous acid was…

A:

Q: Determine the pH of a 0.588 M weak base soultions at 25C. The Kb for the weak base is 1.76 x 10^-5.…

A:

Q: What is the ionization constant at 25 °C for the weak acid CH3 NH3 +, the conjugate acid of the weak…

A: The equilibrium constant for dissociation of a weak acid is called the ionization constant of a weak…

Q: The hydronium ion concentration of an aqueous solution of 0.325 M nitrous acid (Ka = 4.50×10-4) is…

A: Given that -  Molarity of nitrous acid, HNO2 = 0.325 M  Acid dissociation constant, Ka = 4.50×10-4…

Q: Calculate the pH of a 0.14 M HNO2 solution that is 5.7% ionized. Multiple Cholce 2.10 11.90 1.70…

A:

Q: What is the pH of a 75.0mL of a 0.1M pyridine (C5H5N) solution (kb = 1.7 x 10 -9) when 100mL of a…

A:

Q: Calculate the pH of a 0.20M c2h5nh2 solution kb=5.6x10^-4

A: Ethylamine(CH2CH2NH2) is a base (because Ethylamine has one lone pair to accept a proton(H+)).…

Q: Calculate the pH of the following solutions:   a) 1.2 M CaBr2           b) 0.8 M C6H5NH3NO3 (Kb…

A:

Q: Calculate the pH at 25°C of a 0.0047 M solution of a weak base with a K, of 3.5 x 10-9. pH = %3D

A: Answer: Given data: Kb=3.5×10-9C=0.0047M

Q: Calculate the hydronium-ion concentration at 25°C in a 1.3 x 10-2 M Ba(OH)2 solution. Concentration…

A: The Ba(OH)2 dissociates in solution as- Ba(OH)2 (aq)→Ba2+(aq) + 2OH-(aq) Thus, as per balanced…

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.