Compute the pH of the solution after the reaction of 43mL of 0.64M HCN with 3.0...

Compute the pH of the solution after the reaction of 43mL of 0.64M HCN with 3.0 ? 101mL of 0.37 KOH. Part 1: Do the stoichiometry first. HCD(aq)+KOH(AQ) ---> HOH(l) +KCN(aq). a) how many moles of acid and base? b) what is the limiting reactatnt? c) how many moles of excess reactant after the reaction? d) how many moles of pH active product?

Expert Solution

queen_honey_blossom answered 2 years ago

The pH of 0.30 M solution of HCN is 5.20. Calculate the Ka value for HCN.

a. What is the pH of a 0.040 M solution of HCN? Find the concentrations of...

a. What is the pH of a 0.040 M solution of HCN? Find the concentrations of all the major species in the solution? [HCN], [H3O+], [CN-]

What is [H3O+] and pH in a 0.10 M solution of HCN at 25

The pH of a 0.10 M HCN solution is 5.20. a. What is [H3O+ ] in...

The pH of a 0.10 M HCN solution is 5.20. a. What is [H3O+ ] in that solution? _______________ M b. What is [CN-]? What is [HCN]? (Where do the H+ and CN - ions come from?) [CN-] = _______________ M; [HCN] = _____________ M c. What is the value of Ka for HCN? What is the value of pKa? Ka = _______________ pKa = _______________

Part A. Calculate the pH of a buffer solution that is 0.250 M in HCN and...

Part A. Calculate the pH of a buffer solution that is 0.250 M in HCN and 0.168 M in KCN. For HCN, Ka = 4.9×10−10 (pKa = 9.31). Part B. Calculate the pH of a buffer solution that is 0.240 M in HC2H3O2 and 0.190 M in NaC2H3O2. (Ka for HC2H3O2 is 1.8×10−5.) Part C. Consider a buffer solution that is 0.50 M in NH3 and 0.20 M in NH4Cl. For ammonia, pKb=4.75. Calculate the pH of 1.0 L of...

What is the pH of a solution prepared by mixing 25 ml of 0.5 HCN with...

What is the pH of a solution prepared by mixing 25 ml of 0.5 HCN with 75 ml of 0.20 NaCN. Ka = 6.2*10^-10 for HCN. Hint: remember to dilutions first.

Q2: What is the pH and concentration of CN– in a 0.100M solution of HCN? Q3:...

Q2: What is the pH and concentration of CN– in a 0.100M solution of HCN? Q3: What would happen if the equilibrium [CN– ] that you calculated in Q2 was changed by adding 0.00500 moles of solid NaCN to 100.0 mL of the solution? (Which direction is the reaction going to “go” to minimize the disturbance?)

What is the pH of a solution made by dissolving 1.8 g of K2CO3 and 3.0...

What is the pH of a solution made by dissolving 1.8 g of K2CO3 and 3.0 g of KHCO3 in 500. mL of water? Use the Acid-Base Table. Please see Buffer pH for assistance.

The reaction of the weak acid HCN with the strong base KOH is: HCN(aq)+KOH(aq)-->HOH(l)+KCN(aq) To compute...

The reaction of the weak acid HCN with the strong base KOH is: HCN(aq)+KOH(aq)-->HOH(l)+KCN(aq) To compute the pH of the resulting solution if 54mL of 0.79M HCN is mixed with 2.0 × 10^1 mL of 0.32 KOH we need to start with the stoichiometry. Let\'s do just the stoich in steps:. a)How many moles of acid? b)How many moles of base? c)What is the limiting reactant? d)How many moles of the excess reagent after reaction? e)What is the concentration of...

What is [H3O+] and ph in a 0.10 M solution of HCN at 25 degrees celsius...

What is [H3O+] and ph in a 0.10 M solution of HCN at 25 degrees celsius (ka for HCN= 4.0x10-10) show steps

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