HCl and NaOH are strong acid and strong base respectively.
a) HCl + NaOH ------------> NaCl + H2O
At equivalence
mmoles of acid = mmoles of base
30x0.1011 = V x0.09889
Volume of base = 30.67 mL at equivalence
At equivalence as both are strong the pH = 7.00
b)when NaOh volume = 30.67-0.02 = 30.65 mL
HCl + NaOH ------------> NaCl + H2O
30x0.1011=3.033 30.65x0.09889=3.0309 0 0 initial mmoles
0.0021 0 3.0309 --- equilibrium
So the solution is still acidic and [H+] = mmoles/ volume = 0.0021/(30+30.65) =3.46x10-5
pH = -log 3.46x10-5
=4.4606
c) Volume of NaOH = 30.67-0.01 = 30.66 mL
HCl + NaOH ------------> NaCl + H2O
30x0.1011=3.033 30.66x0.09889=3.032 0 0 initial mmoles
0.001 0 3.032 --- equilibrium
So the solution is still acidic and [H+] = mmoles/ volume = 0.001/(30+30.66) =1.65x10-5
pH = -log 1.65x10-5
= 4.7829
d)
when NaOh volume = 30.67-0.02 = 30.65 mL
HCl + NaOH ------------> NaCl + H2O
30x0.1011=3.033 30.69x0.09889=3.0349 0 0 initial mmoles
0 0.0021 3.0309 --- equilibrium
So the solution is basic and [OH-] = mmoles/ volume = 0.0021/(30+30.65) =3.46x10-5
pOH = -log 3.46x10-5
=4.4606
and pH = 14-pOH = 14-4.4606 =9.5394
2. When 30.00 mL of 0.1011 M HCl in 50 ml of Di water is titrated...
1. A 30.00 mL sample of 0.400 M HNO3 is titrated with 0.600 M KOH. What is the balanced neutralization chemical reaction? What volume of base (in mL) must be added to reach the equivalence point? Is the pH of the equivalence point acidic, basic, or neutral?
6)(9) Consider the titration of 30.00 mL 0.300 M HCl(aq) a SA with 0.450 M NaOH(aq) a SB. a) Write an equation for the reaction between HCl and NaOH. b) What volume of NaOH must be added to reach the equivalence point in this titration? c) What is the pll at the equivalence point in this titration (no calculation required)?
A 20 mL sample of 0.01 M propionic acid (CH3CH2COOH; Pka = 4.87) is titrated with 0.05 M NaOH. A) Write out the chemical reaction for this titration. B) Calculate the initial pH of the sample. C) Calculate the volume of NaOH required to reach the equivalence point. D) Calculate the pH of the solution at the equivalence point. E) Sketch a titration curve for this titration (pH versus volume NaOH added). Note the location of the equivalence point on...
An acid-base titration is performed: 250.0 mL of an unknown concentration of HCl(aq) is titrated to the equivalence point with 36.7 mL of a 0.1000 M aqueous solution of NaOH. Which of the following statements is not true of this titration? A. At the equivalence point, the OH−concentration in the solution is 3.67×10−3 M. B. The pH is less than 7 after adding 25 mL of NaOH solution. C. The pH at the equivalence point is 7.00. D. The HCl...
a.)100 mL of 1.00 M HCl solution is titrated with 1.00 M NaOH solution. You added the following quantities of 1.00 M NaOH to the reaction flask. Classify the following conditions based on whether they are before the equivalence point, at the equivalence point, or after the equivalence point/endpoint. 1.) 150 mL of 1 M NaOH 2.) 200 mL of 1 M NaOH 3.) 50 mL of 1 M NaOH 4.) 100 mL of 1 M NaOH 5.) 5.00 mL...
19. The conjugate base salt to a weak acid (NaA) is titrated with 0.100 M HCl to its equivalence point. A 25.0 mL solution of a 0.200 M solution of the salt was titrated. The pK, for the unknown conjugate acid is 4.31. (a) Will the equivalence point be acidic or basic for this titration? i.e. pH less than 7.0 or greater than 7.0? (b) What is the volume in mL needed of HCl to reach the equivalence point? (c)...
Question 2 (20pts): A 20 mL sample of 0.01 M propionic acid (CHsCH2COOH; Pk 4.87) is titrated with 0.05 M NaOH A) Write out the chemical reaction for this titration. B) Calculate the initial pH of the sample. C) Calculate the volume of NaOH required to reach the equivalence point. D) Calculate the pH of the solution at the equivalence point. E) Sketch a titration curve for this titration (pH versus volume NaOH added). Note the Jocation of the equivalence...
A 25.0 mL NaOH solution of unknown concentration was titrated with a 0.189 M HCl solution. 19.6 mL HCl was required to reach equivalence point. In a separate titration, a 10.0 mL H3PO4 solution was titrated with the same NaOH solution. This time, 34.9 mL NaOH was required to reach the equivalence point. What is the concentration of the H3PO4 solution?
2. A 30.00 ml solution of 0.235 M CH2NH2 was titrated with 0.150 M H2S0O.. a) Calculate the pH of the 30.00 ml solution of 0.235 M CH2NH2 The Kb for CH2NH2 is 4.4x 104 b) Calculate the volume of 0.150 M H2S04 required to completely neutralize the 30.00 mL solution of 0.235 M CH2NH2. c)Calculate the volume of 0.150 M H2SO, required to neutralize half the mole of CH2NHz. present 30.00 mL solution of 0.235 M CH2NH2 d) Calculate...
6) A 35 mL solution of 0.241 M HCl is titrated with 0.127 M NaOH: a) How many milliliters of NaOH solution are required to reach the equivalence point? b) What is the pH at the midpoint of the titration? c) What is the pH at the endpoint of the titration?