Calculate [H30+] and [S2-] in a 0.1 M solution of the diprotic acid hydrosulfuric acid. (For...

Calculate [H30+] and [S2-] in a 0.1 M solution of the diprotic acid hydrosulfuric acid. (For hydrosulfuric acid Ka1 = 9.0 times 10-8 and Ka2 = l.OxlO-17.) Enter your answers in scientific notation. [H3O+] = times M [s2-] = times M

Expert Solution

queen_honey_blossom answered 2 years ago

Carbonic acid, H2CO3, is a weak diprotic acid. In a 0.1 M solution of the acid,...

Carbonic acid, H2CO3, is a weak diprotic acid. In a 0.1 M solution of the acid, which of the following species is present in the largest amount? H2CO3. H3O+ HCO3

Calculate the concentration of S2- in an aqueous solution of 0.274 M hydrosulfuric acid, H2S (aq)....

Calculate the concentration of S2- in an aqueous solution of 0.274 M hydrosulfuric acid, H2S (aq). [S2-] = _____ M.

The pH of a solution made of 0.1 M acetic acid and 0.1 M potassium acetate...

The pH of a solution made of 0.1 M acetic acid and 0.1 M potassium acetate is (Ka = 1.8 x 10-5) to which 0.001 mol of KOH has been added: a) pH = 8.92 b) pH = 11.55 c) pH = 4.73 d) pH = 4.74

Calculate pH at equivalence point when 100 mL of a 0.1 M solution of acetic acid...

Calculate pH at equivalence point when 100 mL of a 0.1 M solution of acetic acid (HC2H3O2), which has a Ka value of 1.8 x 10^-5, is titrated with a 0.10 M NaOH solution? Please show your ICE chart and why you chose to use the equations you did.

a) What happens when you add acid to a solution of 0.1 M HNO2 and 0.1...

a) What happens when you add acid to a solution of 0.1 M HNO2 and 0.1 M KNO2? Write a chemical equation if relevant. b) Why doesnt the same kind of reaction occur when you add acid to a solution of 0.1 M HNO3 and 0.1 M KNO3?

a 25.0 mL solution if 0.10 M acetic acid is titrated with 0.1 M NaOH solution....

a 25.0 mL solution if 0.10 M acetic acid is titrated with 0.1 M NaOH solution. the pH equivalence is

1. Calculate the pH of a 0.339 M H2S. Calculate the [S2-] in the solution. 2....

1. Calculate the pH of a 0.339 M H2S. Calculate the [S2-] in the solution. 2. A titration is performed by adding 0.656 M KOH to 40 mL of 0.172 M HNO3: b) Calculate the pH after the addition of 2.1, 5.25 and 9.49 mL of the base.(Show your work in detail for one of the volumes.) e)Calculate the pH after adding 5.00 mL of KOH past the equivalence point

Need to prepare an acetate buffer solution: 25.00 mL of 0.1 M acetic acid and 0.1...

Need to prepare an acetate buffer solution: 25.00 mL of 0.1 M acetic acid and 0.1 M sodium acetate. The stock acetic acid is 6.0 M. The instructions involve the preparation of a (10-fold) intermediate acetic acid solution. Ka = 1.75 x 10-5 (pKa = 4.76). What are the values for the: * volume of acetic acid * grams of sodium acetate (since it's a solid) * volume of DI water needed * calculated pH Thanks.

1. The pH of a solution made of 1.0 M acetic acid and 0.1 M potassium...

1. The pH of a solution made of 1.0 M acetic acid and 0.1 M potassium acetate is (K_a = 1.8 x 10^-5) to which 0.001 mol of KOH has been added: a) pH = 4.74 b) pH = 4.73 c) pH = 8.92 d) pH = 4.46 e) pH = 11.55 The answer is not 4.74!! 2. The pH of a solution made of 1.0 M acetic acid and 0.1 M potassium acetate is (K_a = 1.8 x 10^-5)...

Calculate the molar solubility of barium iodate in a solution that is also 0.1 M in...

Calculate the molar solubility of barium iodate in a solution that is also 0.1 M in KIO3

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