NEET Test Series from KOTA - 10 Papers In MS WORD
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CHXI07:EQUILIBRIUM
314510
Assertion : \(\mathrm{pH}\) of blood is maintained inspite of acidic foods. Reason : Acidity of foods is not so large to change the \(\mathrm{pH}\) of blood.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
Dissolved ratio of \(\mathrm{HCO}_{3}{ }^{-}\)to \(\mathrm{H}_{2} \mathrm{CO}_{3}\) (buffer \(\mathrm{H}_{2} \mathrm{CO}_{3} / \mathrm{HCO}_{3}{ }^{-}\)) is helpful in controlling the \(\mathrm{pH}\) of the blood. So option (3) is correct.
CHXI07:EQUILIBRIUM
314511
The \(\mathrm{pH}\) of blood is 7.4. Assuming that the buffer in blood is carbon dioxide, hydrogen carbonate ion, what is the ratio of conjugate base to acid necessary to maintain blood at its proper \(\mathrm{pH} ?\left(\mathrm{Ka}=4.5 \times 10^{-7}\right)\)
1 9
2 10
3 11
4 12
Explanation:
\(\mathrm {\mathrm{CO}_{2}+2 \mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{H}_{3} \mathrm{O}^{+}+\mathrm{HCO}_{3}^{-}}\) \(\rm {\mathrm{Ka}_{1}=\dfrac{\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\left[\mathrm{HCO}_{3}^{-}\right]}{\left[\mathrm{CO}_{3}^{2-}\right]}=4.5 \times 10^{-7}}\) Given that \(\mathrm {\mathrm{pH}=7.4}\) then \(\mathrm {\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]}\)or \(\mathrm {\left[H^{+}\right]=4 \times 10^{-8}}\) \(\rm {\dfrac{\left[\mathrm{HCO}_{3}^{-}\right]}{\left[\mathrm{CO}_{2}\right]}=\dfrac{4.5 \times 10^{-7}}{4 \times 10^{-8}}=11}\)
CHXI07:EQUILIBRIUM
314512
The \(\mathrm{pH}\) of an acidic buffer mixture is
1 6.8
2 7
3 7.5
4 depends upon \({{\rm{K}}_{\rm{a}}}\) of the acid
Explanation:
The \(\mathrm{pH}\) of acidic buffer is calculated by following formula \(\mathrm{pH}=-\log \mathrm{K}_{\mathrm{a}}+\log \left[\dfrac{\text { salt }}{\text { acid }}\right]\) \(\therefore \mathrm{pH}\) of acidic buffer depends on value of \(\mathrm{K}_{\mathrm{a}}\) and is always less than 7 .
CHXI07:EQUILIBRIUM
314513
Addition of sodium hydroxide solution to a weak acid (HA) results in a buffer of \(\mathrm{pH}\) \({\text{6}}\). If ionisation constant of HA is \(10^{-5}\), the ratio of salt to acid concentration in the buffer solution will be
314510
Assertion : \(\mathrm{pH}\) of blood is maintained inspite of acidic foods. Reason : Acidity of foods is not so large to change the \(\mathrm{pH}\) of blood.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
Dissolved ratio of \(\mathrm{HCO}_{3}{ }^{-}\)to \(\mathrm{H}_{2} \mathrm{CO}_{3}\) (buffer \(\mathrm{H}_{2} \mathrm{CO}_{3} / \mathrm{HCO}_{3}{ }^{-}\)) is helpful in controlling the \(\mathrm{pH}\) of the blood. So option (3) is correct.
CHXI07:EQUILIBRIUM
314511
The \(\mathrm{pH}\) of blood is 7.4. Assuming that the buffer in blood is carbon dioxide, hydrogen carbonate ion, what is the ratio of conjugate base to acid necessary to maintain blood at its proper \(\mathrm{pH} ?\left(\mathrm{Ka}=4.5 \times 10^{-7}\right)\)
1 9
2 10
3 11
4 12
Explanation:
\(\mathrm {\mathrm{CO}_{2}+2 \mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{H}_{3} \mathrm{O}^{+}+\mathrm{HCO}_{3}^{-}}\) \(\rm {\mathrm{Ka}_{1}=\dfrac{\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\left[\mathrm{HCO}_{3}^{-}\right]}{\left[\mathrm{CO}_{3}^{2-}\right]}=4.5 \times 10^{-7}}\) Given that \(\mathrm {\mathrm{pH}=7.4}\) then \(\mathrm {\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]}\)or \(\mathrm {\left[H^{+}\right]=4 \times 10^{-8}}\) \(\rm {\dfrac{\left[\mathrm{HCO}_{3}^{-}\right]}{\left[\mathrm{CO}_{2}\right]}=\dfrac{4.5 \times 10^{-7}}{4 \times 10^{-8}}=11}\)
CHXI07:EQUILIBRIUM
314512
The \(\mathrm{pH}\) of an acidic buffer mixture is
1 6.8
2 7
3 7.5
4 depends upon \({{\rm{K}}_{\rm{a}}}\) of the acid
Explanation:
The \(\mathrm{pH}\) of acidic buffer is calculated by following formula \(\mathrm{pH}=-\log \mathrm{K}_{\mathrm{a}}+\log \left[\dfrac{\text { salt }}{\text { acid }}\right]\) \(\therefore \mathrm{pH}\) of acidic buffer depends on value of \(\mathrm{K}_{\mathrm{a}}\) and is always less than 7 .
CHXI07:EQUILIBRIUM
314513
Addition of sodium hydroxide solution to a weak acid (HA) results in a buffer of \(\mathrm{pH}\) \({\text{6}}\). If ionisation constant of HA is \(10^{-5}\), the ratio of salt to acid concentration in the buffer solution will be
314510
Assertion : \(\mathrm{pH}\) of blood is maintained inspite of acidic foods. Reason : Acidity of foods is not so large to change the \(\mathrm{pH}\) of blood.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
Dissolved ratio of \(\mathrm{HCO}_{3}{ }^{-}\)to \(\mathrm{H}_{2} \mathrm{CO}_{3}\) (buffer \(\mathrm{H}_{2} \mathrm{CO}_{3} / \mathrm{HCO}_{3}{ }^{-}\)) is helpful in controlling the \(\mathrm{pH}\) of the blood. So option (3) is correct.
CHXI07:EQUILIBRIUM
314511
The \(\mathrm{pH}\) of blood is 7.4. Assuming that the buffer in blood is carbon dioxide, hydrogen carbonate ion, what is the ratio of conjugate base to acid necessary to maintain blood at its proper \(\mathrm{pH} ?\left(\mathrm{Ka}=4.5 \times 10^{-7}\right)\)
1 9
2 10
3 11
4 12
Explanation:
\(\mathrm {\mathrm{CO}_{2}+2 \mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{H}_{3} \mathrm{O}^{+}+\mathrm{HCO}_{3}^{-}}\) \(\rm {\mathrm{Ka}_{1}=\dfrac{\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\left[\mathrm{HCO}_{3}^{-}\right]}{\left[\mathrm{CO}_{3}^{2-}\right]}=4.5 \times 10^{-7}}\) Given that \(\mathrm {\mathrm{pH}=7.4}\) then \(\mathrm {\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]}\)or \(\mathrm {\left[H^{+}\right]=4 \times 10^{-8}}\) \(\rm {\dfrac{\left[\mathrm{HCO}_{3}^{-}\right]}{\left[\mathrm{CO}_{2}\right]}=\dfrac{4.5 \times 10^{-7}}{4 \times 10^{-8}}=11}\)
CHXI07:EQUILIBRIUM
314512
The \(\mathrm{pH}\) of an acidic buffer mixture is
1 6.8
2 7
3 7.5
4 depends upon \({{\rm{K}}_{\rm{a}}}\) of the acid
Explanation:
The \(\mathrm{pH}\) of acidic buffer is calculated by following formula \(\mathrm{pH}=-\log \mathrm{K}_{\mathrm{a}}+\log \left[\dfrac{\text { salt }}{\text { acid }}\right]\) \(\therefore \mathrm{pH}\) of acidic buffer depends on value of \(\mathrm{K}_{\mathrm{a}}\) and is always less than 7 .
CHXI07:EQUILIBRIUM
314513
Addition of sodium hydroxide solution to a weak acid (HA) results in a buffer of \(\mathrm{pH}\) \({\text{6}}\). If ionisation constant of HA is \(10^{-5}\), the ratio of salt to acid concentration in the buffer solution will be
314510
Assertion : \(\mathrm{pH}\) of blood is maintained inspite of acidic foods. Reason : Acidity of foods is not so large to change the \(\mathrm{pH}\) of blood.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
Dissolved ratio of \(\mathrm{HCO}_{3}{ }^{-}\)to \(\mathrm{H}_{2} \mathrm{CO}_{3}\) (buffer \(\mathrm{H}_{2} \mathrm{CO}_{3} / \mathrm{HCO}_{3}{ }^{-}\)) is helpful in controlling the \(\mathrm{pH}\) of the blood. So option (3) is correct.
CHXI07:EQUILIBRIUM
314511
The \(\mathrm{pH}\) of blood is 7.4. Assuming that the buffer in blood is carbon dioxide, hydrogen carbonate ion, what is the ratio of conjugate base to acid necessary to maintain blood at its proper \(\mathrm{pH} ?\left(\mathrm{Ka}=4.5 \times 10^{-7}\right)\)
1 9
2 10
3 11
4 12
Explanation:
\(\mathrm {\mathrm{CO}_{2}+2 \mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{H}_{3} \mathrm{O}^{+}+\mathrm{HCO}_{3}^{-}}\) \(\rm {\mathrm{Ka}_{1}=\dfrac{\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\left[\mathrm{HCO}_{3}^{-}\right]}{\left[\mathrm{CO}_{3}^{2-}\right]}=4.5 \times 10^{-7}}\) Given that \(\mathrm {\mathrm{pH}=7.4}\) then \(\mathrm {\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]}\)or \(\mathrm {\left[H^{+}\right]=4 \times 10^{-8}}\) \(\rm {\dfrac{\left[\mathrm{HCO}_{3}^{-}\right]}{\left[\mathrm{CO}_{2}\right]}=\dfrac{4.5 \times 10^{-7}}{4 \times 10^{-8}}=11}\)
CHXI07:EQUILIBRIUM
314512
The \(\mathrm{pH}\) of an acidic buffer mixture is
1 6.8
2 7
3 7.5
4 depends upon \({{\rm{K}}_{\rm{a}}}\) of the acid
Explanation:
The \(\mathrm{pH}\) of acidic buffer is calculated by following formula \(\mathrm{pH}=-\log \mathrm{K}_{\mathrm{a}}+\log \left[\dfrac{\text { salt }}{\text { acid }}\right]\) \(\therefore \mathrm{pH}\) of acidic buffer depends on value of \(\mathrm{K}_{\mathrm{a}}\) and is always less than 7 .
CHXI07:EQUILIBRIUM
314513
Addition of sodium hydroxide solution to a weak acid (HA) results in a buffer of \(\mathrm{pH}\) \({\text{6}}\). If ionisation constant of HA is \(10^{-5}\), the ratio of salt to acid concentration in the buffer solution will be
