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If the $ K_b $ value in the hydrolysis reaction $ B^+ + H_2 O \rightleftharpoons BOH + H^+ is 1.0 \times 10 ^ {-6} $ then hydrolysis constant of salt would be
For a sparingly soluble salt $ A_pB_q relation ship of its solubility product(K_{SP})$ with its solubility(s) is.
$ ApBq_{(s)} \rightleftharpoons PA^{q+}_(aq) + q B ^{p-} _{(aq)} $ Solubility is PS qS mol/lit $K_{SP} = (PS) ^ P \times (qs) ^ q$ $ = S^ (p+q) \times P^P \times q^ q $
How many grams $ CaC_2O_4 (mw = 128) on dissolving in distill water will give saturated solution [K_{SP} = (CaC_2O_4 ) = 2.5 \times 10 ^ {-9} mol^2 l^{-2 } $
To find the amount of CaC_2O_4 that will dissolve to form a saturated solution, we use the solubility product constant ( extit{K}{sp}). For CaC_2O_4, extit{K}{sp} = 2.5 imes 10^{-9}. The solubility (s) can be found from extit{K}_{sp} = s^2, giving s = rac{1}{2} imes 10^{-4.5}. The molar mass of CaC_2O_4 is 128 g/mol. Therefore, the mass of CaC_2O_4 that will dissolve in 1 liter of water is s imes 128 = 0.0064 g.
If the concentration of $ CrO_4 { 2–} ion ina saturated solution of silver chromate is 2 \times 10 ^ {-4} $ solubility product of silve chromate will be
The equilibrium is:
According to bronsted- lowryconcept. correct order of relative strength of bases follows the order
According to the Bronsted-Lowry concept, base strength is determined by the ability to accept protons. The hydroxide ion (OH^-) is a stronger base than acetate (CH_3COO^-) and chloride (Cl^-). Thus, the correct order of base strength is OH^- > CH_3COO^- > Cl^-.
$ HSO_4 ^ - + OH ^ - \rightarrow SO^{2-} _ 4 + H_2O $ Which is correct about conjugate acid base pair
In the given reaction, $HSO_4^- ightarrow SO_4^{2-} + H_2O$, $HSO_4^-$ acts as an acid as it donates a proton (H^+), and $SO_4^{2-}$ is its conjugate base. Thus, $SO_4^{2-}$ is the conjugate base of the acid $HSO_4^-$. This is because in a conjugate acid-base pair, the acid has one more proton (H^+) than its conjugate base.
Which of following base is weakest
The strength of a base is determined by its $K_b$ value. A lower $K_b$ value indicates a weaker base. Given the $K_b$ values:
HClO is a weak acid. concentration of $ H^+ ion in 0.1 M solution of HClO (Ka = 5 \times 10^{-8} ) $ will be
$ Co = 0.1 M Ka = 5 \times 10 ^{-8} $ $ [H ^ + ]= \sqrt {Ka.CO} $ $ = (5 \times 10 ^ {-8} \times 0.1) ^{ 1/2} = (50 \times 10 ^ {-10} ) ^ {1/2} = 7.07 \times 10 ^ {-5 } M. $
$ NH_4Cl$ is acidic because
$NH_4Cl$ is acidic because, upon hydrolysis, it gives a weak base ($NH_4OH$) and a strong acid (HCl). The hydrolysis reaction is: $NH_4Cl + H_2O ightarrow NH_4OH + HCl$ Since $HCl$ is a strong acid and completely dissociates in water, it makes the solution acidic.
100 ml of 0.04 N HCl aqueous solution is mixed with 100 mlof 0.02 N NaOH solution. The $ P^H $ of resulting solution is
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