Find the pH of 0.175 M NaCN solution. For HCN,Ka = 4.9 * 10-10.a) 5.03 b) 11.28 c) 2.31 d) 8.97

Q: Hydrocyanic acid, HCN, is a weak acid (Ka = 4.02*10-10). If I dissolve 0.882 g of HCN in enough…

A: Given information is as follows: The amount of HCN = 0.882 g The volume of water = 600 mL The value…

Q: 19) Calculate the pH of a solution (aq., 25 °C) prepared by dissolving 48.026 g of ammonium nitrate…

A: Given:   Mass of NH4NO3=48.026g   Molar mass of NH4NO3=80.043 g/mol   Volume =2.00L…

Q: Calculate pH of the following solutions: a) 0.25 M HNO3 in 0.065 M CH3COOH (K,=1.75x10). b) 0.33 M…

A:

Q: If the formic acid (HCO2H) Ka is 1.8 × 10-4, then the pH of a 0.35 M solution of sodium formate…

A: Here we are are required to find the pH of the solution of sodium formate.

Q: Calculate the pH of each solution.(a) [H3O+] = 1.7 * 10-8 M(b) [H3O+] = 1.0 * 10-7 M(c) [H3O+] = 2.2…

A:

Q: Calculate the pH of a solution

A:

Q: Find the pH of a 0.350 Maqueous benzoic acid solution. For benzoic acid, K, = 6.5 x 10-5. a) 4.64 b)…

A: The dissociation of benzoic acid is as follows:      C6H5COOHaq    ↔ H+aq+ C6H5COO-I       0.350…

Q: a) Find the pH of a 0.110 M solution of a weak monoprotic acid having Ka= 1.0×10−5. b) Find the…

A: GivenThe molarity of the solution = 0.11MKa = 1.0 x 10-5

Q: Determine the pH of a 0.50 M NaF solution. The Ka of HF is 3.5 x 10-5. Enter the result to 2 decimal…

A:

Q: 5) if 125.0 ml water is added to 175.0 ml a strong acid solution of PH = 3. What should be the PH of…

A: Molarity : It is one of unit of the measurement of the concentration of a solution. It is defined as…

Q: What is the pH of 0.15 M solution of acetic acid (CH3COOH) Ka=1.75 x 10^-5 A) 2.6 x 10^-6 B) 0.0016…

A: Calculating pH of the acetic acid. CH3COOH + H2O <----------> CH3COO- + H3O+

Q: Questions 30 and 31 both involve a 0.22 M solution of acetic acid (CH3COOH). Tme Ka of CH3COOH is…

A:

Q: 14. When 0.1 mol of a salt is dissolved in 1.0 L of solution, the pH of the solution is 8.07. What…

A:

Q: 4) Aniline, (C6H5NH2, Kh = 4.3 x 10-10 Determine the pH of an aniline solution made by dissolving…

A: Calculate the molarity of aniline,

Q: Butyric acid, C3H;COOH, has ionization constant of 1.54 x 10-5. a) Calculate the pH of 50.0 mL of a…

A:

Q: What is the pH of a solution prepared by mixing 50.00mL of 0.10 M NH3 with 10.00 mL of 0.10 M NH4Cl?…

A: Given data is as follows:

Q: What is the pH of a solution that is 0.33 M CH3NH2 (methylamine) and 0.52 M CH3NH3Cl (methylammonium…

A: Since we have weak base CH3NH2 and its conjugate acid CH3NH3Cl in the solution. Hence the solution…

Q: Benzoic acid, C6H5COOH, is a weak acid (Ka = 6.28*10-5). If I dissolve 1.22 g of C6H5COOH in enough…

A: Molarity of benzoic acid (M)= No of moles / Volume in Liter No of moles = Mass / molar mass = 1.22 /…

Q: Arsenic acid (HAs04) is a triprotic acid with Ka1 = 5.5x10-3, Ka2 = 1.7×10-7, and Ka3 = 5.1x10-12.…

A:

Q: QUESTION 1 In a NaOH solution [OH-] is 2.9 x 10-4M. Calculate the pH of the solution. (Round-off…

A: Note: As per our guidelines, we are supposed to answer the first question when multiple questions…

Q: Determine the pH of the following solutions. a) 0.29 mol L-1 KNO2 (Ka(HNO2) = 5.6 x 10-4) b) 0.21…

A:

Q: Calculate pH of the following solutions: 0.25 M HNO3 in 0.065 M CH COOH (K.=1.75x10).

A: Solution: We know the common ion aslo affect on oH of the solution. Here first we need to draw an…

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: Determine the pH of a 0.50 M NaF solution. The Ka of HF is 3.5 × 10-5. Enter the result to 2…

A: The concentration of the salt, NaF is = 0.50 M The dissociation constant of Hf is = 3.5 × 10-5 The…

Q: 2. Consider the weak acid phenol (C6H5OH), for which Ka = 1.05 x10-10 in aqueous solutions at 5°C.…

A: Given:  Concentration of phenol (C) = 0.850 M  Ka = 1.05 x 10-10

Q: 7. Calculate [H3O+] and [OH-] for each solution of either a strong acid or a strong base. Calculate…

A: Since you have posted a question with multiple sub-parts ,we will solve the first three sub-parts…

Q: Q1) Calculate the KbKb value for CH3COO−CH3COO−. Q2) Calculate the KbKb value for CN−CN−. Round…

A: Ka and Kb values of a weak acid/conjugate base or weak base/conjugate acid pair are related through…

Q: a) What is the pH of a solution prepared by adding 11.1 mL of 0.50 M NaOH solution to 200. mL of a…

A: The question is based on the concept of buffer solution.   A buffer is a solution which resist any…

Q: Whats pH of a solution that is 0.010 M in HClO Ka = 3.5 × 10–8 and 0.010 M in HCl?

A: Since HCl is a strong acid, it is completely dissociated into H+(aq) and Cl-(aq).  Hence [H+(aq)] =…

Q: What is the pH of 0.1M solution of weak acid having ionization constant (Ka) is 10 A) 7 B) 6. C) 4…

A:

Q: This question has two parts. Part-I (a) Calculate the pH of a 0.20 M HF solution. The Ka of HF is…

A: Part-I (a)  A 0.20 M HF solution. The Ka of HF is 6.8*10-4. Determine pH of solution ?       Part-II…

Q: What is the pH of 8.1 x 10-5 M HCIO4 solution? a) 4.09 Ob) 9.91 Oc) -4.09

A: pH = - log[H+]

Q: What is the pH of a solution that is 0.11 M CH3NH2 (methylamine) and 0.15 M CH3NH3Cl (methylammonium…

A: Since the solution is having weak base CH3NH2 and its conjugate acid salt CH3NH3Cl  Hence the…

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.