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Consider titrating 100.0 ml of 0.100 M HCOOH with unknown volume of 0.100 M of Sr(OH)2....
Consider the titration of 100.0 mL of 0.100 M methylamine (CH3NH2) with 0.500 M HNO3. Calculate the pH at the following volumes of acid added. For CH3NH3+, pKa = 10.632 (a) Find the equivalence point volume. (b) 0 mL (c) 9.0 mL (d) 10.0 mL (e) 20.0 mL (f) 30.0 mL
Consider the titration of 100.0 mL of 0.200 M CH3NH2 by 0.100 M HCI (K for CHNH2 4.4 x 10) At what volume of HCl added, does the pH 10.64? XmL
Consider the titration of 100.0 ml of 0.200 M CH3NH2 by 0.100 M HCl. (Kb for CH3NH2 = 4.4 x 10^-4) At what volume of HCl added, does the pH = 10.64?
ANSWER NUMBER 9 ONLY
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pH Ht! B C mL of titrating reagent in buret → We were unable to transcribe this image9. For the titration of 100.0 mL of 0.0500 M NH, with 0.100 M HCI, the curve will look different he diagram on the other side of this page (see your answer to question 7). Considering the than t points to be in corresponding places to the curve presented for question 8, calculate parts a-f from...
B. Simone is titrating 80.00 mL of 0.120 M HIO (in the flask) with 0.100 M NaOH (in the buret). Calculate the pH when 75.00 mL of 0.100 M NaOH has been added.
100.0 mL of 0.100 M sodium sulfide is mixed with 100.0 mL of 0.100 M chromium (III) nitrate. Calculate the mass of solid that forms and the concentration of the remaining species in solution: assume complete precipitation.
Calculate the change in pH when 3.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3 (aq) and 0.100 M in NH4CI(aq). Consult the table of ionization constants as needed ДрН Calculate the change in pH when 3.00 mL of 0.100 M N2OH is added to the original buffer solution. АрН -
Consider a solution formed by mixing 60.0 mL of 0.100 M H2SO4, 39.9 mL of 0.100 M HOCl, 30.0 mL of 0.200 M NaOH, 30.0 mL of 0.100 MCa(OH)2, and 12.7 mL of 0.150 M KOH. Calculate the pH of this solution.
Consider the titration of 40.0 mL of 0.200 M HCIO4 by 0.100 M KOH. Calculate the pH of the resulting solution after the following volumes of KOH have been added. a. 0.0 mL pH = b. 10.0 mL pH = c. 60.0 mL pH = d. 80.0 mL pH = e. 110.0 mL pH = Consider the titration of 100.0 mL of 0.200 M acetic acid (Ka = 1.8 x 10-5) by 0.100 M KOH. Calculate the pH of the...
Consider the titration of 100.0 mL of 0.100 M /hydrazine () by 0.200 M . Assume that hydrazine is monoprotic. Determine the following: a. pH before any HNO3 is added b. volume of acid to reach the equivalence point c. pH when 20.0 mL of HNO3 has been added d. pH when 25.0 mL of HNO3 has been added e. pH when 40.0 mL of HNO3 has been added f. pH when 50.0 mL of HNO3 has been added g....