HCN ionises to give H+ ion and CN- ion.
HCN --------> H+ + CN-
0.100 M HCN will contain 0.100 M H+ ion.
Concentration of H+ ion = 0.100 M
Find the pH of a 0.100 M carbonic acid (H2CO3) solution. Find the equilibrium concentration of CO3 -2. Ka1 = 4.30 x 10-7 Ka2 = 5.59 x 10-11
Calculate the pH of 0.65 M NaCN. What is the concentration of HCN in the solution? PH= [HCN]= Times 10 M
Calculate the concentration of all species present in a solution that is 0.025 M in HCN and 0.010 M in NaOH (Ka (HCN) = 4.9×10^-10)
The pH of a solution of 0.100 M HCN, given Ka= 4.9 X 10^-10 is Answer is supposed to be 5.5, but I'm not sure why
3. A 40.00 mL 0.100 M solution of HCN was slowly titrated with 0.200 M NaOH solution. Complete the following table and show your calculations in the space provided. Volume of NaOH added (mL) pH 0.00 5.00 10.00 15.00 20.00 25.00 Show your calculations for pH clearly and in steps.
A 0.100 M solution of HCNO has a [H+] of 0.0045 M. A 0.100 M solution of CH3COOH has a [H+] of 0.0013 M. a) Which acid should have a larger numerical value for KA? Defend your answer to get credit. No math needed – just explain. b)Which acid should have a larger numerical value for KB? No math needed, just explain. c)Which acid should have a larger numerical pKA? d)What is the pOH of the CH3COOH solution (want a...
2.) 100.0 mL of a 0.100 M solution of HCN (K,=4.9 10-19) is titrated with a 0.200 M solution of KOH. Calculate the pH of solution iii) Before any addition of KOH solution. (2pts) After the addition of 10.0 mL of KOH solution. (2pts) At the half-equivalence point. (1pt) At the equivalence point. (2pts) After the addition of 100 mL of KOH solution. (1pt)
What concentration of NaCN must be added to a 0.5 M HCN solution to produce a buffer solution with pH 7.0? Ka = 6.2 x 10–10 for HCN a) 3.3 M b) 0.49 M c) 6.9 x 10-5 M d) 0.0031 M e) 0.22 M
What are the concentrations at equilibrium of a 0.15 M solution of HCN? What will be the concentration of Cu2+(aq) at equilibrium? HCN(aq)<=>H+(aq) + CN–(aq) , Kc= 4.9 x 10-10
Calculate the concentration of cyanide (CN–) in a 0.450 M solution of hydrocyanic acid HCN and 0.10M –10 HCl. [For HCN, Ka = 6.2 × 10] a. 0.1M b. 2.8×10–9M c. 7.8×10–5M d. 1.1×10–6M e. 0.21 M with steps please