Question

What is the pH of a 0.280 M solution oof
H_{2}SO_{4}? K_{a2} =1.2 x
10^{-2}

^{Please help and show work, thank you}

Answer #1

What is the pH of a 0.260 M solution of H2SO4? Ka2 =
1.20×10^–2?
Please write out steps if possible so that I can understand,
thank you!

1) What is the ph of a 0.005 M , solution of h2so4?
ka2=1.2x10^-2 of HSo4-

Determine the pH of a 0.034 solution of H2SO4. The
dissociation occurs in two steps. Ka1 is extremely large; Ka2 is
1.2 * 10^-2
Please show work thanks

What is the pH of a 0.170 M solution of sulfurous acid? Given:
Ka1 = 1.70×10–2, Ka2 = 6.20×10–8 Please show the setup of the
quadratic if possible. Thank you in advance!

What is the pH of a 0.20 M solution of disodium hydrogen
phosphate? Ka2 = 6.2 x 10^- 8and Ka3 = 2.2 x 10^-1 3

What is the pH of 0.40 M Na2SO3? (K1 for H2SO3 = 1.5 x 10^-2; K2
= 1.0 x 10^-7). Correct answer is 10.30. Please show work to show
why this is the correct answer. Thank you!

Calculate the pH of 0.15 M H2SO4(aq) at 25◦C, given that Ka1 is
very large and Ka2 = 1.2 × 10−2

Calculate the [H3O+] and pH of each H2SO4 solution. At
approximately what concentration does the x is small approximation
break down? Ka2 = 0.012
a. 0.50 M
b. 0.10 M
c. 0.050 M
What does "x is small approximation" mean? Also, I have no idea
how to solve for x for part a and probably the other so please do
not skip a step... I was trying to solve it and I had no idea why
it went from 0.012...

a) What is the pH of 0.10 M NaH2PO4?
Ka2 = 6.2 x 10-8
b) What is the pH of 0.10 M Na2HPO4?
Ka3 = 2.2 x 10-13

what is the pH of a 0.300 M solution of
H2SO4

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