e. 2.0 x 108 M 1. The pH of a solution is 4.80. What is the concentration of hydroxide ions in this solution? c. 3.6 x 10-12 M a.4.2 x 100 M b. 1.6 x 105 M d. 6.3 x 10-10 M
States of Matter
The substance that constitutes everything in the universe is known as matter. Matter comprises atoms which in turn are composed of electrons, protons, and neutrons. Different atoms combine together to give rise to molecules that act as a foundation for all kinds of substances. There are five states of matter based on their energies of attraction, namely solid, liquid, gases, plasma, and BEC (Bose-Einstein condensates).
Chemical Reactions and Equations
When a chemical species is transformed into another chemical species it is said to have undergone a chemical reaction. It consists of breaking existing bonds and forming new bonds by changing the position of electrons. These reactions are best explained using a chemical equation.
![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
d 8.52
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 NaClO4 d. NH3 and (NH4)2SO4
d. 5.5
e. 2.0 x 10-8 M
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
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
9. what will happened to the pH of buffer system when it diluted
a. ApH=0
b. pH will increased c. pH will decrease d. pH >7 e.
e.7.00
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
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
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
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
d. 9150ppm
a. 243 ppm
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
c. 3.76
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%2F0f942feb-24ba-4611-8ad3-396dbc50eb06%2F6xhknxg_processed.jpeg&w=3840&q=75)
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