HCl dissociates completely to give H+
The concentration of H+,
[H+] = [HCl] = 0.150 M
use below formula to calculate pH:
pH = -log [H+]
= -log (0.150)
= 0.82
Answer: D
s) Question 11 (2 point An aqueous solution contains 0.150 M HCI at 25.0 °C. The...
An aqueous solution contains 0.250 M HCl at 25.0 °C. The pH of the solution is OA 0.150 B. 1.00 OC 13.00 O 0.0.60 €. 0.82
will you show me how to do #18? ) Of the following substances, an aqueous solution of NH4CI Cu(NO3)2 K2CO3 NaF will form basic solutions. A) NH4CI, Cu(NO3)2 D) NaF, K2CO3 B) K2CO3, NH4CI E) NH4CI only C) NaF only Answer: D 17) A 0.1 M aqueous solution of NaOCI KCI NH4CI Ca(OAc)2 will have a pH of 7.0 at 25.0°C. A) NaOCI D) Ca(OAc)2 B) KCI E) KCI and NH4C C) NH4C Answer: B 18) What is the pH...
2. Consider an aqueous solution comprised of 0.200 M NH3 and 0.150 M NHACI. The pKb of NH3 is 4.75 and the volume of the solution is 1.00 L. a) (2 marks) What is the pH of this solution? Show your work. b) (1 mark) What is the chemical reaction (balanced chemical equation) that occurs when NaOH solution is added to the original solution? c) (3 marks) How many moles of NaOH(s) could this solution react with before its pH...
please answer both questions QUESTION 18 An aqueous solution contains 0.27 M ammonium chloride, NH4Cl. One liter of this solution could be converted into a buffer by the addition of 1.0.27 mol NH4Br 6.0.27 mol HBC 6.0.13 mol HCI 1.0.26 mol NH3 9.0.26 mol KCI QUESTION 19 A 29.9 ml. sample of 0.299 M methylamine, CH3NH2, is titrated with 0.331 M hydroiodic acid, HI at 25°C. (Xb for methylamine is 4.2 * 10-4) What is the pH at the equivalence...
A 25.0 mL sample of 0.150 M chloroacetic acid is titrated with a 0.150 M NaOH solution. What is the pH at the equivalence point? The of chloroacetic acid is 1.4 ×10-3.
Consider an aqueous solution comprised of 0.150 M NH3 and 0.200 M NH4Cl. The pKb of NH3 is 4.75 and the volume of the solution is 1.00 L. a) What is the pH of this solution? Show your work. b) What is the chemical reaction (balanced chemical equation) that occurs when NaOH solution is added to the original solution? c) How many moles of NaOH(s) could this solution react with before its pH rises to 10.00? Show your work.
QUESTION 11 How many nitrate ions are present in 25.0 mL of 0.150 M copper(ll) nitrate solution? e a 0.00750 ions b.4.52 x 1021 ions 12.01 x 1023 ions 2.26 x 1021 tons QUESTION 12 Draw the Lewis structure for NO2, including any resonance structures. Based on the meaning of resonance struc of the nitrite anion? a. It contains 2 single bonds D.It contains 2 bonds of equivalent length, of bond order intermediate between a single and double bond. C.It...
A 50.00 mL sample of a 0.150 M aqueous solution of a weak acid HA is titrated with a 0.300 M aqueous solution of NaOH. At which point in the titration will the pH of the solution equal pKa of the acid? a) After addition of 50.00 mL of the NaOH solution b) After addition of 25.00 mL of the NaOH solution c) After addition of 12.50 mL of the NaOH solution d) After addition of 6.25 mL of the...
Exam review questions 2) In which aqueous system is PbF2 least soluble? 2) A) 1.0 M HNO3 B) H20 C) 0.5 M HF D) 0.2 MHF E) 0.8 M KF 3) A buffer solution contains 0.100 M fluoride ions and 0.126 M hydrogen fluoride. What is the 3) concentration (M) of hydrogen fluoride after addition of 7.00 mL. of 0.0100 M HCI to 25.0 mL of this C0.123 4) In which of the following aqueous solutions would you expect AgCl...
QUESTION 11 Calculate the pH for an aqueous solution of acid that contains 2.15 x 10-3 M H30 at equilibrium. A. 4.65x 10-12 B. 2.15 x 10-3 11.33 Oc OD. 2.67 QUESTION 12 Calculate the pH for an aqueous solution that contains 2.15 x 10-3 M OH at 25 °C A. 4.65 x 10-11 B.2.15x 10-4 O c.3.67 OD. 11.33