2017年3月30日 · KCN is the salt of a strong base (KOH) and a weak acid (HCN), and thus the salt in aqueous solution will have a basic pH. One needs to then look at the hydrolysis of the cyanide anion, CN^-, which is as follows:

2023年10月20日 · KCN is the salt of a strong base (KOH) and a weak acid (HCN). Thus, the pH of the solution should be >7 (basic). To find the pH of 0.0315 M KCN solution, we need to look at the hydrolysis of CN - :

2021年10月6日 · Since both reactants are aqueous (aq), and the product KCN is aqueous and all are strong electrolytes (ionize completely), the only species that we need to be concerned with is the liquid H 2 O(l). This is true for many acid/base reactions where the products are a salt and water. H + (aq) + OH-(aq) ==> H 2 O(l) ... NET IONIC EQUATION

2021年4月30日 · Calculate the ph of a buffer solution that is 0.250 M HCN and 0.170 M KCN. Ka=4.9x10^-10 for HCN. A) add 0.099 mol NaOH to calculate the new ph B) add 10 ml of 1.00 M HCl and calculate the new ph

Adoria L. asked • 10/17/20 When a 4.00 g sample of KSCN is dissolved in water in a calorimeter W/ total heat capacity of 2.85 kJ⋅K−1, the temperature decreases by 0.350 K. Calculate the molar heat of solution of KSCN.

2020年10月19日 · pH = -log[H +] so we need to find the [H +]. HCN ==> H + + CN-. Ka = 4.9x10-10 = [H +][CN-]/[HCN]. 4.9x10-10 = (x)(x)/(0.0740 - x) and if we assume x is small ...

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