A is not true. You would LIKE about 10^5 difference in k1 and k2 but usually we can live with 10^3(1000 times) and in some cases even 10^2 (100 time) but never as close as 10^1 (10 times)
I don't believe B is true but the statement isn't really all that clear to me.
C is not true.
D is true if we're talking diprotic acids. Probably not true true for triprotic acids.
E is generally true.
F is not true. k2 is ALWAYS smaller than k1.
What simplifying assumptions do we usually make in working problems involving equilibria of salts of polyprotic acids? Why are they usually valid? Answer by selecting all true statements.
Are the answers: a,b,d,and f
A)If the two ionization constants are not very different the approximations are valid.
B)The concentration of OH- and the conjugate acid of the weak base (the anion of the salt) are approximately equal.
C)Nearly all of the OH- comes from the first ionization.
D)Nearly all of the OH- comes from the second ionization.
E)The approximations are usually valid because the first ionization constant is usually much larger than the second ionization constant.
F)The approximations are usually valid because the first ionization constant is usually smaller than the second ionization constant.
2 answers
c) Nearly all of the OH- comes from the first ionization.
e) The approximations are usually valid because the first ionization constant is usually much larger than the second ionization constant.
b) The concentration of OH- and the conjugate acid of the weak base (the anion of the salt) are approximately equal.
e) The approximations are usually valid because the first ionization constant is usually much larger than the second ionization constant.
b) The concentration of OH- and the conjugate acid of the weak base (the anion of the salt) are approximately equal.
1 answer