A solution has a pH of 4.75: is the solution, acidic, basic or neutral? what is

Question

A solution has a pH of 4.75: is the solution, acidic, basic or neutral? what is the [H+] ion concentration of the solution? what is the pOH and the [OH-] ion concentration of the solution? And; would the pH increase, decrease or remain the same if some water is added to the buffer? A 0.10 M solution of lactic acid, a weak monoprotic acid of formula HC_3H_5O_3, was found to have a pH of 2.43. What is the value of K_a for the acid? What is the pH of a 0.20 M aqueous solution of acetic acid, CH_3COOH? Ka for acetic acid = 1.8 times 10^=5. What is the pH of a 0.15 M aqueous solution of ammonia? Kb for ammonia is 1.8 times 10^-5. Calculate Ka for the anilinium ion given that Kb for aniline (C6H5NH2) is 1.5 times 10_-10 Calculate Kb for the cyanide ion given that Ka for HCN(aq) is 1.5 times 10_-10 What is the pH of a solution that is 0.25 M in formic acid (HCOOH) and 0.15 M in sodium formate? Ka for formic acid is 4.4 times 10-4. Give a recipe for preparing a acetate buffer solution having a pH of 3.60. Ka for acetic acid is 1.8 times 10-5. A saturated solution of silver chromate (Ag_2CrO_4) was found to have a CrO_42- ion concentration of 3.2 times 10_-4 M at 25 degree C. What is the K_sp for Ag_2CrO_4? Calculate the molar solubility of AgCl in 0.100 M sodium chloride given that K_sp for silver chloride for is 1.6 times 10-10. Calculate the solubility of CaCO_3 (molar mass 100.0 g/mol) in mg/L in water given K_sp is 4.7 times 10-9.

Explanation / Answer

1.At a pH of 4.75,the solution is acidic solution.

Calculate the H+ as follows:

pH = = log [H+]

[H+]=10^-4.75=0.0000177

pOH=-log[OH-]

pH+pOH=14

pOH=14-4.75=9.25

[OH-=10^-9.25=5.62*10^-10

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