Researchers have shown that hypochlorous acid (HCIO) generated by white blood cells kills bacteria. The Ka of this acid is 2.9 X 10-8 a) What is the pH of 0.40 M HCIO? b) What is the percent dissociation of 0.40 M HCIO?

Q: The statements below apply to acid A and base B. • Neutral salts are formed when acid A reacts with…

A: Given: Concentration of base B = 2.13×10-3 M the pH of a solution of base B = 11.6

Q: 3) Aniline (B), shown below, is an organic base used in the manufacture of certain plastics. NH2 a)…

A: Given,   aniline is represented by B it is given that it is a base.

Q: An acid (HA) dissociates as follows: HA – H* + A minus Arrow should be interpreted as an equilibrium…

A: The equilibrium reaction given is, => HA --------> H+ + A-  Given : Initial concentration of…

Q: An acid (HA) dissociates as follows: HA → H* + A minus Arrow should be interpreted as an equilibrium…

A: Given :-  HA <-----> H+ + A-  Initial concentration of HA = 0.37 M  pH = 4.91   To be…

Q: If the K of a weak base is 8.5 x 10-6, what is the pH of a 0.27 M solution of this base? pH =

A:

Q: 4. a. If 0.457 g of NH3 are dissolved in enough water to make 500. mL of solution, what is the pH of…

A: First calculate molarity of ammonia by Mole divide by volume. [OH-]=√kb×C And Dissociation = √kc÷C

Q: 4- A solution is prepared by adding 50.0 mL of 0.050 M HBr to 150.0 mL of 0.10 M HI. Calculate [H*]…

A: [H+] and pH of the solution is to be calculated.

Q: Ka= 1.76 x 10-5 for HC2H3O2 What is the pH of this solution? Table 1 Solution Buffer solution acetic…

A:

Q: What is the pH of a solution that results from mixing together equal volumes of a 0.130 M  solution…

A: Given, 0.130 M solution of acetic acid 0.065 M solution of sodium hydroxide pKa of acetic acid =…

Q: Hydrofluoric acid (HF) has a Ka value of 7.2 x 10-4. What is the pH to 2 decimal places when 6.875…

A: When weak acid HF reacts with KOH to form a buffer solution . The pH of buffer solution can be…

Q: What is the pH of a 80.0 mL solution which is 0.23 M in IO and 0.47 M in HIO? The Ka for HIO is 2.3…

A: When a weak acid(eg HIO) mixed with its conjugate base (ege IO-) they form a buffer solution. pH of…

Q: A 0.100 M solution of the salt BHX has a pH of 8.00, where B is a weak base and X- is the anion of…

A: As per the given information BHX is dissociate in solution to produce BH+and X- ions. because the…

Q: What is the pH of a 0.139 M solution of HF? Ka for Hf is 6.6 x 10-4

A:

Q: What will the concentrations be for a, b, and c?  What is the pH of the solution?

A: Concentration = moles/volume.[pyridine] =mol/volume = 0.3mol/1 L = 0.3M.

Q: What is the pH value of 1x10-3 M CH3COOH solution? (Ka: 1.75x10-5)

A:

Q: How much 0.573 M KOH will be needed to raise the pH of 0.215 L of 3.23 M carbonic acid (H2CO3) to a…

A: Carbonic acid and base both are acid and base so will give salt  Resultant solution is Acidic…

Q: Hydrofluoric acid (HF) is a weak acid with a Ka = 7.1 x 10-4. What is the pH of a 0.50 M solution of…

A: Given acid is a weak acid, so it will not completely dissociate into products.Construct ICE table…

Q: A generic base, B¯, is added to 30.00 L of water. The pH of the solution is found to be 9.05. What…

A: The hydrogen ion [H+] concentration in the solution having a pH of 9.05 is calculated as shown…

Q: What is the pH of a solution that is 0.75 M HF and 0.15 M NaF?   The Ka of HF is 6.6 x 10-4

A: Given: Concentration of HF [HF]= 0.75 M Concentration of NaF [NaF]= 0.15 M Ka of HF is 6.6 x 10-4 To…

Q: If the Ka of a monoprotic weak acid is 3.4 × 10-6, what is the pH of a 0.30 M solution of this acid?

A: The dissociation of a weak acid is written as:

Q: Calculate the pH of a 0.30 M solution of HCN (weak acid). Ka for HCN is 4.9 x 10-10

A: Given: Concentration of the HCN solution = 0.30 M Ka for HCN = 4.9 × 10-10 We have to calculate the…

Q: What is the pH of a 0.10 M NaF solution? The Ka for HF is 6.8 x 10-4

A: The values are given as follows:

Q: For the diprotic weak acid H2A, Kaj = 3.1 x 10-6 and Ka2 = 8.9 x 10-9. What is the pH of a 0.0550 M…

A:

Q: 1.) HA is a weak acid. Its ionization constant, Ka, is 3.1 x 10-13. Calculate the pH of an aqueous…

A: 1)  The ionization constant for the weak acid is = 3.1 x 10-13 The initial NaA concentration is =…

Q: HA is a weak acid. Its ionization constant, Ka, is 2.4 x 10-13. Calculate the pH of an aqueous…

A: Given : The solution has salt NaA with concentration 0.063 M Since NaA is an ionic salt. Hence it…

Q: A weak acid (HA) solution has a 5.6 x 10-5 M of H3O*. If the Ka for the weak acid is 3.1 x 10-8

A: We have to calculate the initial concentration of weak acid.

Q: Lemons get their sour flavor from citric acid (Ka = 7.4 x 10-4) a fresh squeezed lemon can have a…

A:

Q: A solution contains 0.020 M CsBrO, what is the pH of the solution? Ka (HBRO) = 2.8x10-9

A: Given the Ka of HBrO = 2.8×10-9 We have to calculate the pH of a solution that contains 0.020 M…

Q: What is the pH of a solution that results from mixing together equal volumes of a 0.120 M  solution…

A:

Q: What is the pH of a solution that contains 0.2 M HCN and 0.1 M Ba(CN)2? The Ka for HCN is 6.2x10-10

A: Given Molarity of HCN = 0.2 MMolarity of Ba(CN)2 = 0.1 MKa(HCN) = 6.2 * 10-10pH = To be determined

Q: 1.) HA is a weak acid. Its ionization constant, Ka, is 3.1 x 10-13. Calculate the pH of an aqueous…

A: Answer:- This question is answered by using the simple concept of calculation of weak acid and the…

Q: a) What is the pH and pOH of 0.001 M NaOH solution, which is the strong base? b) The Ka value of…

A: pH + pOH = 14 pOH = -log [OH-] For a weak acid: [H+] = (Ka x C)1/2 Where, C = molar concentration

Q: If the Ka of a monoprotic weak acid is 8.3 × 10-6, what is the pH of a 0.19 M solution of this acid?

A: Given, Concentration of monoprotic weak acid = 0.19 M Ka of monoprotic weak acid = 8.3 × 10-6

Q: What is the pH of a 80.0 mL solution which is 0.27 M in IO and 0.49 M in HIO? The Ka for HIO is 2.3…

A:

Q: You add 100.0 mL of 0.10 M KOH to 50.0 mL of 0.20 M HCIO. What is the pH of the resulting solution?…

A: Given: 100mL of 0.10M KOH 50mL of 0.20M HClO

Q: Hydrofluoric acid (HF) has a Ka of 7.4×10 . If 0.500 M HF is present in a flask, what is the pH of…

A:

Q: What will be the H+ concentration in a 0.25 M solution of a weak acid (HA), of Ka = 6.9x10-3 What…

A:

Q: 5. The pH of a 0.035 M solution of a weak acid, HX, is 4.25. (a) Calculate Ka for HX and (b)…

A: The pH of a 0.035 M solution of a weak acid, HX, is 4.25. a) Ka for HX and b) the percent ionization…

Q: If the K of a weak base is 2.4 x 10-6, what is the pH of a 0.47 M solution of this base? pH =

A:

Q: A solution of a weak acid, HA, has [HA] = [A-] = 0.301 M.  If the acid dissociation constant for the…

A: Given: [HA] = [A-] = 0.301 M Acid dissociation constant, Ka = 2.2 x 10-4

Q: What is the pH of a 0.010 M solution of HF? The Ka for HF is 6.8 x 10^-4.

A: Given,   Concentration of HF = 0.010 M  Ka for HF is = 6.8x10-4

Q: If the Ka of a monoprotic weak acid is 1.3 x 10-6, what is the pH of a 0.18 M solution of this acid?…

A:

Q: If the Ka of a monoprotic weak acid is 1.6 x 10-6, what is the pH of a 0.37 M solution of this acid?…

A:

Q: What is the hydronium ion concentration in 0.0200 M HClO?   Ka = 2.88 x 10-8

A: In order to calculate the concentration of the hydronium ion we first write down the given data:…

Q: The Ka of a weak monoprotic acid is 1.13 x 10-5. What is the pH of a 0.0777 M solution of this acid?…

A:

Q: If the Ka of a monoprotic weak acid is 4.7 x 10-6, what is the pH of a 0.49 M solution of this acid?…

A: Given Ka = 4.7 x 10-6 C = 0.49 M

Q: What is the pH of the solution of 50 mL of 0.25 M HCN after 20 mL of 0.10 M NaOH has been added?…

A: Volume of HCN = 50 ml  Molarity of HCN = 0.25 M  Volume of NaOH = 20 ml Molarity of NaOH= 0.10 M…

Q: What is the pH of a solution that is 0.025M formic acid, HCHO2, and 0.018M sodium formate,…

A:

Q: 6) What is the hydronium ion concentration of a 0.010 M solution of acetic acid? Ka for acetic acid…

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.