7.77. Assertion: Higher order ionization constants (Ka2, Ka3) are higher than the lower order ionization constant (Ka1) of a polyprotic acid.
Reason: It is more difficult to remove a positively charged proton from a negative ion due to electrostatic forces.
7.77. Assertion: Higher order ionization constants (Ka2, Ka3) are higher than the lower order ionization constant (Ka1) of a polyprotic acid.
Reason: It is more difficult to remove a positively charged proton from a negative ion due to electrostatic forces.
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1 Answer
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(d) Higher order ionization constants (Ka2, Ka3) are smaller than the lower order ionization constant (Ka1) of a polyprotic acid. The reason for this is that it is more difficult to remove a positively charged proton from a negative ion due to electrostatic forces. This can be seen in the case of removing a proton from the uncharged H2CO3 as compared from a negatively charged HCO3–.Similarly, it is more difficult to remove a proton from a doubly charged HPO42– anion as compared to H2PO4–.
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0.01 M NaOH,
M = 1 * 10-2
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Kc = 0.36 * 0.0821 * 300 = 8.86 » 9
A(g) ->B(g) + (g)
Initial moles n 0 0
Eqb. moles n(1 – a) na
total moles =
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