As #Mg (OH)_2# is a base weaker of ammonia it doesn't react with #NH_4Cl# #NH_4Cl# whose pH is # [H^+]= sqrt (K_w/K_b xx Cs)=sqrt (10^ (-14)/ (1,8 xx10^ (-5))xx 1= 2,3 xx 10^-5# that is …

The balanced chemical equation for the partial dissociation of the base looks like this "BOH"_text ( (aq]) rightleftharpoons "B"_text ( (aq])^ (+) + "OH"_text ( (aq])^ (-) By definition, K_b will be …

OH− (aq) + H3O+ (aq) → 2H2O(l) so you can say that when you mix these two solutions, the hydronium cations present in the hydrochloric acid solution will be the limiting reagent, i.e. they …

The acid in excess is then titrated with N aOH (aq) of KNOWN concentration....we can thus get back to the concentration or molar quantity of M (OH)2...as it stands the question (and answer) …

"6.3072 g" >>"Molarity" = "Moles of solute"/"Volume of solution (in litres)" "0.45 M" = "n"/"0.4 L" "n = 0.45 M × 0.4 L = 0.18 mol" You need "0.18 mol" of "NH"_4"OH" Molar mass of "NH"_4"OH" …

The degree of dissociation sf (alpha=0.0158) sf (K_b=2.51xx10^ (-6)color (white) (x)"mol/l") Triethyamine is a weak base and ionises: sf ( (CH_3)_3N+H_2Orightleftharpoons …

Aug 29, 2016 · So this is a propanol derivative: "2-methylpropan-2-ol" For "isopropyl alcohol", H_3C-CH (OH)CH_3, the longest chain is again three carbons long, and C2 is substituted by …

Similarly, OH^- becomes H_2O, indicating a gain of a H^+ ion. So, you can say that NH_4^+ is the acid, and OH^- is the base. Conjugates are basically the "other" term. For every acid, you …

See explanation... Roughly speaking, we have the following facts: [H_3O^+] * [OH^-] = 10^(-14) pH = -log_10 [H_3O^+] pOH = -log_10 [OH^-] { (pH < 7 " acidic"), (pH ...

On the product side the Carbonic Acid (#H_2CO_3#) is the Conjugate Acid as it is the hydrogen donor to the Conjugate Base (#OH^-#) as it receives the hydrogen ion.