A buffer solution is made that is 0.423 M in and 0.423 M in . If for is , what i
ID: 1037050 • Letter: A
Question
A buffer solution is made that is 0.423 M in and 0.423 M in .
If for is , what is the pH of the buffer solution?
pH =
Write the net ionic equation for the reaction that occurs when 0.086 mol is added to 1.00 L of the buffer solution.
(Use the lowest possible coefficients. Omit states of matter. Use instead of )
A buffer solution is made that is 0.314 M in H2S and 0.314 M in NaHS. If Kai for H2S is 1.00 x 10-7, what is the pH of the buffer solution? pH Write the net ionic equation for the reaction that occurs when 0.093 mol KOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.)
Explanation / Answer
2. use the henderson hasselbach equation:
PH = PKa + log [salt]/[acid]
pka = - log (Ka) = - log ( 1 x 10-7) = 7
PH = 7 + log (0.423 / 0.423) = 7 + 0 = 7
B)
H2S + NaOH = NaHS + H2O, this is the chemical, equation, separate the compounds into ions to get the total ionic equation:
H2S + Na+ + OH- === Na+ + HS- + H2O
remove the terms that appear on both sides of the equation:
H2S + OH- === HS- + H2O , this is the net ionic equation.
*hope you find it useful =)
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