4-Which of the following combinations cannot produce a buffer solution? a. HNO2 and NaNO₂ b. HCN and NaCN c. HCIO4 and NaClO4 d. NH3 and (NH4)2SO4 e. NH3 and NH4Br
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
![1. The pH of a solution is 4.80. What is the concentration of hydroxide ions in this solution?
a.4.2 x 10 M b. 1.6 x 105 M
c. 3.6 x 10-12 M
d. 6.3 x 10-10 M
2 the pH of a 0.50 M solution of NaNO₂. Ka for HNO₂ is 4×10-5
a 12.1
b. 5.48
c. 1.82
c. 8.90
3- What was the pH of the solution that result from titration of 25.0 ml of 0.5 M solution of weak base (Kb - 9.74×10) wi
30 ml of 0.1 M hydrochloric acid, HCI.?
a. 5.10
b. 4.92
d. 9.1
4-Which of the following combinations cannot produce a buffer solution?
a. HNO2 and NaNO₂ b. HCN and NaCN c. HCIO4 and NaCIO4 d. NH3 and (NH4)2SO4
d. 5.5
e. 2.0 x 10-8 M
d 8.52
e. NH3 and NH4Br
5- What is the pH at the equivalence point in the titration of 100.0 mL of 0.20 M ammonia (NH3) with 0.10 M
hydrochloric acid (HCI)? Kb for NH31.8x 10-5
a. 4.6
b. 5.2
c. 7.0
e. 4.9
9. what will happened to the pH of buffer system when it diluted
a. ApH=0
b. pH will increased c. pH will decrease
e.7.00
6- If 10.00 ml of 0.1M NaOH solution is needed to reach the end point of 10 ml HNO3. Then the concentration of HNO3 in
ppm is: [M.wt. of HNO3= 63 g/mol]
e. 25.77 x 10³ ppm
a. 9.45×10³ ppm
b.14.70 x10³ ppm
c. 6.30 × 10³ ppm
d. 18.77 × 10¹ ppm
7. A 0.6745-gram sample of KHP reacts with 41.75 mL of KOH solution for complete neutralization. What is the
molarity of the KOH solution? (Molecular weight of KHP = 204 g/mol. KHP has one acidic hydrogen.)
a. 0.158 M
c. 0.139 M
b. 0.099 M
d. 0.079 M
e. 0.061 M
13. The molar analytical concentration of NO
were added to 20.0 ml of 0. 82 M Fe (NO3)2
a.1.09M
b. 2.53 M
8. Which of the following combinations would give a pH =7.00 at the "equivalence point" (when equal moles of each have
been added)?
a. HCI + KF
b. HCN + NaOH
c. HF + HCI
d. HCI + KOH
d. pH >7 e.
pH = 7
10. the pH for Acidic buffer system with highest capacity if the Ka for the weak Acid 1.8 104 is
a. 4.3
b.5.3
c.3.77
d.6.8
e. 8.3
c.0.73 M
e. 9.5
c. 3.76
11. The ppm concentration of Cl-ion in 100 ml mixture solution of 0.01 M CaCl2 and 0.1 M HCI is (MW of Cl =
35.45 g/mol and for Cl =35.45 g/mol ) is :-
b. 4254 ppm
c. 355 ppm
a. 243 ppm
d. 9150ppm
e. 850ppm
from the primary-
12. The mass of AgNO3(s) needed to prepare 1.000 L of 0.0500 M AgNO3 (169.87 g/mol) solution
standard-grade solid is
a. 18.548g
b. 16.987 g
c. 16.139 g
d. 9.843g
e. 10.36 g
ions in the solution produced when 25.0 ml of Distilled water
d. 0.11 M
14. Standard solution of EDTA (0.100 M) is being used to titrate 25.00 ml of (0.0100) M of Zn²+ solution (buffered
at pH =10, 04-0.36 and kMY = 3.2x10¹6) the pZn after the addition of 25 ml EDTA solution is (at equivalent
point)
a. 8.68
b. 9.03
d. 9.79
e. 0.13 M
e. 6.89](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F46ef3182-b77b-4d5e-aa39-bd37ce4fcd02%2F9b197549-ec47-44e8-971e-d31995baef76%2Fpxsca3_processed.jpeg&w=3840&q=75)
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