Which one of these responses is true with regard to a 0.1 M solution of a...

Which one of these responses is true with regard to a 0.1 M solution of a weak acid HA? EXPLAIN WHY D IS RIGHT

A) [OH–] > [H+]

B) [H+] < [A–]

C) [H+] >[A–]

D) pH > 1.0

E) pH = 1.0

Expert Solution

Weak acid does not dissociate completly.

HA H⁺ + A^-

A) [OH-] > [H+] says solution is basic, which is not true because it is an acid solution by dissociation of weak acid.

B) [H+] < [A-] this is not true because the number of H+ and A- ions are same as they are formed by dissociation of one molecule of HA.

C) [H+] < [A-] this is also not true reason as above.

D) pH >1.0 Yes this ti true as it is a weak acid and heance it will have pH>1.

E) pH=1.o this is not nesscesorly true. As acid is a weal acid and hence pH could be around 3-5.

Thus answer is D).

queen_honey_blossom answered 2 years ago

Given a 0.1 M NH4Cl solution: a) Which is the pH of this solution? b) If...

Given a 0.1 M NH4Cl solution: a) Which is the pH of this solution? b) If 100 mL of 0.1 M HCl solution are added to 100 mL of the original solution, which is the pH? c) And if 100 mL of 0.1 M NH3 are added to 100 mL of the original solution? Data: kb(NH3 ) = 1.8 10^-5 .

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

Which one of the following will act as a buffer solution? A. 25 ml of 0.1...

Which one of the following will act as a buffer solution? A. 25 ml of 0.1 M NH4Cl solution mixed with 12.5 mL of 0.1 M NaCl solution B. 25 mL of 0.1 M NH4Cl solution mixed with 25 mL of 0.1 M NaOH solution C. 25 mL of 0.1 M HCl solution mixed with 12.5 mL of 0.1 M NaCl solution D. 12.5 mL of 0.1 M acetic acid solution mixed with 25 mL of 0.1 M NaOH solution...

A buffer solution is prepared by making a solution 0.1 M in NH3 and 0.2M in...

A buffer solution is prepared by making a solution 0.1 M in NH3 and 0.2M in NH4Cl. a) Write the equation for the ionization of NH3 in water. b) Write the expression for the ionization constant, Kb, for NH3. The value of Kb at 25 celsius is 1.8E-5. c) Calculate the [OH-], the [H+], and the pH for this buffer solution. d) Calculate the [OH-], the [H+], and the pH for 0.1 M NH3.

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

Which of the following is true with regard to a SWOT analysis?

Which of the following is true with regard to a SWOT analysis?It classifies SBUs into four distinct categories.It measures customer response to a new product.It evaluates the company's overall strengths.It evaluates the growth potential of a market segment.It ignores the threats faced by a company while assessing its situation in the market.

A system contains a 0.1 molar solution of NaCl and a 0.01 M solution of NaCl...

A system contains a 0.1 molar solution of NaCl and a 0.01 M solution of NaCl separated by an oherise impermeable membrane hat contains a special sodium-conducting pore called an ionophore. The 0.1M solution is inside the membane and the 0.01 Molar solution is outsie the membrane. This ionophore allows free diffusion of the Na+ ions, but not Cl- ions. T=300K, R= 8.31 J/K/mol, F= 96500 J/mol/volt... a) what is the total chemical potential difference, that includes concentration dependent potential...

Which of these has the lower concentration of hydrogen ions: 0.1 M H2SO4, 0.1 M HCl,...

Which of these has the lower concentration of hydrogen ions: 0.1 M H2SO4, 0.1 M HCl, CaCO3, or pure water?

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.

Question