JEE Main 2024 (Online) 1st February Evening Shift | Ionic Equilibrium Question 5 | Chemistry

JEE Main 2024 (Online) 1st February Evening Shift

MCQ (Single Correct Answer)

-1

Solubility of calcium phosphate (molecular mass, M) in water is $\mathrm{W_{g}}$ per $100 \mathrm{~mL}$ at $25^{\circ} \mathrm{C}$. Its solubility product at $25^{\circ} \mathrm{C}$ will be approximately.

$10^7\left(\frac{W}{M}\right)^3$

$10^3\left(\frac{\mathrm{W}}{\mathrm{M}}\right)^5$

$10^7\left(\frac{W}{M}\right)^5$

$10^5\left(\frac{\mathrm{W}}{\mathrm{M}}\right)^5$

JEE Main 2024 (Online) 27th January Morning Shift

MCQ (Single Correct Answer)

-1

Given below are two statements :

Statement (I) : Aqueous solution of ammonium carbonate is basic.

Statement (II) : Acidic/basic nature of salt solution of a salt of weak acid and weak base depends on $$K_a$$ and $$K_b$$ value of acid and the base forming it.

In the light of the above statements, choose the most appropriate answer from the options given below :

Both Statement I and Statement II are correct

Statement I is correct but Statement II is incorrect

Both Statement I and Statement II are incorrect

Statement I is incorrect but Statement II is correct

JEE Main 2023 (Online) 15th April Morning Shift

MCQ (Single Correct Answer)

-1

Which of the following statement(s) is/are correct?

(A) The $\mathrm{pH}$ of $1 \times 10^{-8}~ \mathrm{M} ~\mathrm{HCl}$ solution is 8 .

(B) The conjugate base of $\mathrm{H}_{2} \mathrm{PO}_{4}^{-}$ is $\mathrm{HPO}_{4}^{2-}$.

(C) $\mathrm{K}_{\mathrm{w}}$ increases with increase in temperature.

(D) When a solution of a weak monoprotic acid is titrated against a strong base at half neutralisation point, $\mathrm{pH}=\frac{1}{2} \mathrm{pK}_{\mathrm{a}}$

Choose the correct answer from the options given below:

$(\mathrm{A}),(\mathrm{B}),(\mathrm{C})$

(B), (C)

(B), (C), (D)

(A), (D)

JEE Main 2023 (Online) 11th April Morning Shift

MCQ (Single Correct Answer)

-1

$$25 \mathrm{~mL}$$ of silver nitrate solution (1M) is added dropwise to $$25 \mathrm{~mL}$$ of potassium iodide $$(1.05 \mathrm{M})$$ solution. The ion(s) present in very small quantity in the solution is/are :

$$\mathrm{I^-}$$ only

$$\mathrm{K^+}$$ only

$$\mathrm{Ag^+}$$ and $$\mathrm{I^-}$$ both

$$\mathrm{NO_3^-}$$ only

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