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Solid $ Ba (NO_3)_2 $ is gradually dissolved in 1.0 $ \times 10 ^{-4} M Na_2CO_3 $ solution. At what concentration of will precipitate Ksp of $ BaCO_3 = 5.1 \times 10 ^ {-9} $
$ K_{SP} of BaCo_3 = [Ba^{2+} ][CO^{2-} _3] $ $ \therefore [Ba ^{2+} ] = { 5.1 \times 10 ^ {-9} \over 1 \times 10 ^ {-4} } = 5.1 \times 10 ^ {-5} M $
What is the $ [OH ^-] in the final solution prepared by mixing of 20.0 ml of 0.05 M HCl with 30.0 ml of 0.1 M Ba (OH)_2$ (?)
$ Ba(OH)_2 + 2HCl \rightarrow BaCl_2 + 2H_2O $ 2 mol HCl neutralize1 mole $ Ba(OH)_2 $ $ \therefore 1mol HCl neutralize0.5 mole Ba(OH)_2 $ $ Ba(OH)_2 \rightarrow Ba^{2+}+ 2OH ^ - $ 1 2 $ \therefore no.of molesof Ba(OH)_2 = 3 = 1 +2 $ $ \therefore Ba(OH)_2 left = 3 - 0.5 = 2.5 $ $ \therefore [ Ba(OH)_2 ] = { 2.5 \over 50 } = 0.05 M $ $ or [ OH^ - ] = 2 \times 0.05 M = 0.1 M $
The ionisation constant of NH4OH is1.77 ï‚´10ï€5 at 298 k. Hydrolysis constant of it is
$ K_h = { K_w \over K_b } = { 1.0 \times 10 ^ {-14} \over 1.7 \times 10^{-5} } = 5.65 \times 10 ^ {-10} $
The dissociation constant of a substituted benzoic acid at $ 25 ^\circ C is 1.0 \times 10 ^{-4}. The P^H $ of 0.01 M solution of its sodium salt is
$ P ^ H = + { 1 \over 2 } ( P ^K W + P ^K a + log C ) $ $ = 1/2 \times 14 + 1/2 \times 4 + 1 /2 log 10 ^ {-2} $ = 7+2 -1 = 8
Number of $ H ^+ ions present in 500 ml of lemon juice of P ^ H = 3 $ is
$ P^H = 3 means [H^+] = 10 ^{-3} M $ 1000 ml juice contains $ 10 ^ {-3 }mole H ^ + $ ions $ \therefore no.of H ^ + ions = 10 ^{-3} \times 6.022 \times 10^{23} $ in 1000 ml $ 500 ml juice contains H^+ ions = { 10 ^{-3 } \times 6.022 \times 10^{23} \times 500 \over 1000} $ $ = 3.011 \times 10 ^ {20} $
Equimolar solution of the following were prepared in water separately. Which one of the solutions will record the highest $ P^H $ (?)
All alkaline earthmetalchlorides $ MCl_2$ on hydrolysis will produce acidic solution $ MCl_2 + H_2O \rightleftharpoons M(OH)_2 + 2HCl $ because $ M(OH)_2$ is a weak base and HCl is a strong acid. but as we go down the group, basic character of hydroxides increses. Hence acidic character decreses. So $ BaCl_2 will have the highest P^H$ .
Solubility products constants (KSP) of the salt types $ MX, MX_2 and M_3X at temp T. are 4 \times 10 ^{-8} , 3.2 \times 10 ^{-14 } and 2.7 \times 10 ^{-15} $ respectively. Solubility of the salts at temp. T are in the order,
$ MX_{(S)} \rightleftharpoons M ^ + + X ^ - $ $ K_{SP} = S^2 \therefore S = (K_{SP}) ^ {1/2} = (4 \times 10^ {-8} ) ^ {1/2} = 2 \times 10 ^ {-4} M $ $ MX_{2(s)} \rightleftharpoons M^{2+} + 2 X ^ - K_{SP} = 4 S ^3 \therefore S = ( { K_{SP} \over 4 } ) ^ {1/3} = 2 \times 10 ^ {-5} M $ $ M_3 X_{(s)} \rightleftharpoons 3M^+ + X^ {-3} $ $ K_{SP} = 27 S^4 \therefore S = ( { K_{SP} \over 27 } ) ^ {1/4 } = ( { 2.7 \times 10 ^ {-15} \over 27 } ) ^ {1/4 } = 1 \times 10 ^ {-4} M $ $ \therefore 2 \times 10 ^ {-4} \gt 1 \times 10 ^ {-4} \gt 2 \times 10 ^ {-5 } $ $ \therefore MX \gt M_3 X \gt MX_2 $
When $ H ^ + $ ion concentration of a solution increases
The pH of a solution is a measure of the concentration of hydrogen ions ($H^+$). When the concentration of $H^+$ ions increases, the pH value decreases because pH is the negative logarithm of the $H^+$ ion concentration (pH = -log[H+]).
The aqueous solution of $ HCOO Na, C_6H_5 NH_3Cl, and KCN $ are respectively
HCOONa is a Salt of weak acid (HCOOH) and Strong base (NaOH) So it is basic. $ C_6H_5NH_3Cl is a Salt of weak base (C_6H_5 NH_2 )$ and strong acid (HCl) so it is acidic. KCN is a Salt of Strong base (KOH) and weak acid (HCN) so it is basic.
$ K_{SP} of AgIO_3 is 1 \times 10 ^ {-8} $ at a given temperature what is the mass of $ AgIO_3 $ in 100 ml of its saturated solution ?
$ AgIO_{3(g)} \rightleftharpoons Ag ^ + _{(aq)} + IO ^- _{3(aq)} $ $ K_{SP} = S^2 $ $ \therefore S = { K_{SP} ) ^ {1/2} = (1.0 \times 10 ^ {-8} ) ^ {1/2} = 1 \times 10 ^ {-4} mol /lit $ $ \therefore S = 1 \times 10 ^ {-4} \times 283 = 283 \times 10 ^ {-4} gm/ lit $ $ 1000 ml contains 283 \times 10 ^ {-4} gm of AgIO_3 $ $ 100 ml contains 28.3 \times 10 ^{-4} gm of AgIO_3 $
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