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The solution which tends to keep the con...

The solution which tends to keep the concentration of hydrogen ions constant even when small amount of strong acid or strong base are added to them, is known as

A

Acidic solution

B

Alkaline solution

C

Buffer solution

D

Ideal solution

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The correct Answer is:
C
Buffer solutions maintain the concentration of hydrogen ions constant even when small amounts of strong acid or strong base are added to them.
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A solution which remains in equilibrium with undissolved solute is said to be saturated. The concentration of a saturated solution at a given temperature is called solubility. The product of concentration of ions in a saturated solution of an electrolyte at a given temperature, is called solubility product (K_(sp)) . For the electrolyte, A_(x),B_(y),:A_(x),B_(y(s)) rarr xA^(y+)+ y^(Bx-) , with solubility S, the solubility product (K_(sp)) =x^(x)xxy^(y) xx s^(x+y) . While calculating the solubility of a sparingly soluble salt in the presence of some strong electrolyte containing a common ion, the common ion concentration is practically equal to that of strong electrolyte. If in a solution, the ionic product of an clectrolyte exceeds its K_(sp) , value at a particular temperature, then precipitation occurs. The solubility of BaSO_(4) , in 0.1 M BaCl_(2) , solution is (K_(sp) , of BaSO_(4), = 1.5 xx 10^(-9))

A solution which remains in equilibrium with undissolved solute is said to be saturated. The concentration of a saturated solution at a given temperature is called solubility. The product of concentration of ions in a saturated solution of an electrolyte at a given temperature, is called solubility product (K_(sp)) . For the electrolyte, A_(x),B_(y),:A_(x),B_(y(s)) rarr xA^(y+)+ y^(Bx-) , with solubility S, the solubility product (K_(sp)) =x^(x)xxy^(y) xx s^(x+y) . While calculating the solubility of a sparingly soluble salt in the presence of some strong electrolyte containing a common ion, the common ion concentration is practically equal to that of strong electrolyte. If in a solution, the ionic product of an clectrolyte exceeds its K_(sp) , value at a particular temperature, then precipitation occurs. The solubility of PbSO_(4) , in water is 0.303 g/l at 25^(@) C, its solubility product at that temperature is

When a salt reacts with water to form acidic (or ) basic solution the process is called salt hydrolysis. The P^(H) of salt solution can be calculated using the following relation P^(H) =(1)/(2) [P^(k_w) +P^(Ka) + log C ] for salt of weak acid and strong base. P^(H) =(1)/(2) [P^(K_w) -P^(K_a) -log C ] for salt of weak base and strong acid , P^(H) =(1)/(2) [P^(K_w) +P^(K_a) - P^(K_b) ] For a salt of weak acid and weak base where .c. represents the concentration of salt . When a weak acid (or) a weak base is not completly neatralised by strong base (or ) strong acid respectively, then formation of buffer takes places. The P^(H) of buffer solution can be calculated using the following relation P^(H) =P^(Ka) +log "" ((["salt")])/(["Acid "]) , P^(OH) =P^(Kb) +log ""(["salt"])/(["base"]) Answer the following questions using the following data pK_a (CH_3COOH) =4.7447 , pK_b (NH_4OH) =4.7447 , P^(K_W) =14. One mole CH_3 COOH and one mole CH_3 COONa are dissolved in water one litre aqueous solution The P^(H) of the resulting solution will be

When a salt reacts with water to form acidic (or ) basic solution the process is called salt hydrolysis. The P^(H) of salt solution can be calculated using the following relation P^(H) =(1)/(2) [P^(k_w) +P^(Ka) + log C ] for salt of weak acid and strong base. P^(H) =(1)/(2) [P^(K_w) -P^(K_a) -log C ] for salt of weak base and strong acid , P^(H) =(1)/(2) [P^(K_w) +P^(K_a) - P^(K_b) ] For a salt of weak acid and weak base where .c. represents the concentration of salt . When a weak acid (or) a weak base is not completly neatralised by strong base (or ) strong acid respectively, then formation of buffer takes places. The P^(H) of buffer solution can be calculated using the following relation P^(H) =P^(Ka) +log "" ((["salt")])/(["Acid "]) , P^(OH) =P^(Kb) +log ""(["salt"])/(["base"]) Answer the following questions using the following data pK_a (CH_3COOH) =4.7447 , pK_b (NH_4OH) =4.7447 , P^(K_W) =14. 0.001 M NH_4 Cl aqueous solution has P^(H)

SIA PUBLICATION-CHEMICAL EQUILIBRIUM AND ACIDES-BASES-MCQ
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  2. Which of the following is least likely to act as a Lewis base?

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  3. Which of the following is not a Lewis acid?

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  4. The equilibrium constant (K(C)) for the reaction HA +B hArr BH^(+) + A...

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  5. In the equilibrium reaction, A(g) + 2B(g) + (g), the equilibrium const...

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  6. The ionic product of water is 10^(-14). What is the hydrogen ion conce...

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  7. The pH of a 0.05 M solution of H(2)SO(4) is

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  8. The pH of a 0.001 M aqueous solution of sodium hydroxide will be

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  9. The nature of 0.1 M solution of sodium bisulphate is

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  10. The ionic product of water [H^(+)][OH^(-)] is

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  11. The solution which tends to keep the concentration of hydrogen ions co...

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  12. In the reaction H(2)(g) + Cl(2) (g) rarr 2HCI(g), relation between K(p...

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  13. If in 100 mL of an aqueous HCI of pH 10, 900 mL of distilled water is ...

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  14. The degree of dissociation of an acid HA in 0.1 M solution is 0.1%. It...

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  15. The pH of 10^(-2) M NAOH solution is,

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  16. The solution that is made by mixing appropriate amount of a weak acid ...

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  17. The pK(a) of a certain weak acid is 4.0. What should be the [salt] to ...

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  18. The conjugate base of HSO(4)^(-) ion is ……..

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  19. Aqueous solution of FeCl(3) is acidic because of

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  20. 0.1 M HCI solution is diluted by 100 times. The pH of the solution so ...

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