Molarity

Q. The molarity of $98\%$ $H_{2}S{O}_4$ $(d=1.8\frac{g}{ml})$ by weight is :

1. $6M$
2. $18M$
3. $10M$
4. $4M$

Q. Conc H2SO4 is 98%by mass and has density of 1.84g cm-3 what volume of conc acid is required to make 5l of .5 M H2SO4

Q. Find the density of a 3.6 M sulphuric acid solution i.e 29% H2SO4 by mass

Q. The amount of anhydrous $N{a}_{2}C{O}_3$ present in 250 mL of 0.25 M solution is:

1. $6.625g$
2. $66.25g$
3. $12.68g$
4. $24.35g$

Q. 6. The average molar mass of a mixture of CO(g) and CO2(g) is 37.The mole percentage of CO(g) in the mixture is approximately

Q.

What Molarity Is 85% Phosphoric Acid?

Q.

The pH of ${10}^{-8}$ M HCl solution is

1. slightly less than 7

2. 0

3. 8

4. 7

Q. The folowing reaction 2Br^{- } + Cl_2 → 2cl^- + Br_2 is used for the commercial preparation of bromine from its salts. suppose we have 50 ml of a 0.080 M solution of NaBr. what volume of a 0.050 M solution of Cl_2

Q.

What volume of 0.50 M $CaC{l}_2$ solution is needed to prepare 250 mL of solution that has a chloride concentration of 0.100 M?

Q.

The molarity of the solution containing 2.8% mass-volume solution of KOH. (Given atomic mass of K = 39) is

1. 1 M

2. 0.5 M

3. 0.2 m

4. 0.1 M

Q. Calculate the number of oxalic acid molecules in $100mL$ of $0.02N$ oxalic acid.

1. $6.023\times {10}^{20}$
2. $6.023\times {10}^{21}$
3. $6.023\times {10}^{22}$
4. $6.023\times {10}^{23}$

Q. Which of the following is dependent on temperature?

1. Molality
2. Molarity
3. Mole fraction
4. Weight percentage

Q. 28 kg of N2 and 3 kg of H2 are mixed to produce NH3. The maximum amount of NH3 formed is.

Q. The mass of potassium dichromate (294 g/mol)required to oxidise 750 cm3 of 0.6 M Mohrssalt solution is:-(1) 0.49 g(3) 22.05 g59.(2) 0.45 g(4) 2.2 g

Q.

Number of moles of hydroxide ions in 0.3L of 0.005M solution of Ba (OH)₂ is:

1. 0.0075

2. 0.0015

3. 0.0050

4. 0.003

Q. What volume of water must be added to $50\text{mL}$ of a $0.5M{H}_{2}S{O}_4$ to give a solution having a concentration of $0.1M{H}_{2}S{O}_4?$

1. $200\text{mL}$
2. $250\text{mL}$
3. $105\text{mL}$
4. $550\text{mL}$

Q. explain: mole fraction is independent of the temperature because it does not contains volume term. explain the term "volume term "also.

Q. the average molar mass of CO and CO2 of the mixture is 37.the mole percentage of C

Q. The amount of water obtained on burning 10 gm of H2 in 40 gm of O2 is

Q. The ratio of moles of $N{a}_{2}C{O}_3$ to total number of moles in a 100 mL aqueous solution of $N{a}_{2}C{O}_3$ is 1:5. If 90 g of water is present in 100 mL of solution, find the molarity of the solution.

1. 12.5 M
2. 1.2580 M
3. 0.0125 M
4. 0.1538 M

Q. A concentrated solution of sulphuric acid is 98% $H_{2}S{O}_4$ by mass and has a density of 1.84 g/mL. What volume of this concentrated acid solution is required to make 5 L of a 9.2 M $H_{2}S{O}_4$ solution?
(Molar mass of $H_{2}S{O}_4$ = 98 g/mol)

1. 6.5 L
2. 1.7 L
3. 2.5 L
4. 3.2 L

Q. Find the molarity of a solution made by mixing equal volumes of 30% by weight of $H_{2}S{O}_4$ (density = 1.218 g/mL) and 70% by weight of $H_{2}S{O}_4$ (density = 1.610 g/mL) solutions.

1. 1.48 M
2. 7.61 M
3. 5.83 M
4. 9.25 M

Q. pH of 0.01 M $H{S}^{-}$ will be -

1. =

2. =

3. =

4. =

Q. 200 mL of a 1 M $HN{O}_3$ solution is mixed with 300 mL of 6 M $HN{O}_3$ and the final solution is diluted to 1000 mL. Calculate the concentration of $H^{+}$ ions.

1. 2 M
2. 1 M
3. 4 M
4. 6 M

Q. If 200 mL of a standard 0.15 M NaOH solution is required to neutralize 30 ml of $H_{2}S{O}_4$, what is the molarity of acid?

1. 1.0 M
2. 2.0 M
3. 0.5 M
4. 1.5 M

Q. Find the strength of 500 mL of a 1 M glucose solution.

1. 90 g/L
2. 45 g/L
3. 180 g/L
4. 135 g/L

Q. 38.200 gm of CaCO3 are taken in a 4L container at a certain temperature.Kc for the dissociation of CaCO3 at this temperature is found to be 1/4moleL-1. Then the concentration of CaO(s) in mole/litre is (Given density of CaO=1.12gcm-3) OPTIONS: A)1/2 B)1/4 C)0.02 D)20

Q. $100{\text{cm}}^3$ of a 0.1 M $HCl$ solution is mixed with $100{\text{cm}}^3$ of a 0.2 N $NaOH$ solution. The concentration of excess reagent left and the nature of resulting solution is:

1. Molarity = 0.1 M and the solution is basic
2. Molarity = 0.1 M and the solution is acidic
3. Molarity = 0.05 M and the solution is basic
4. Molarity = 0.05 M and the solution is acidic

Q. A solution of $H_{2}S{O}_4$ has a strength of 4.9 g/L. Find the molarity of the solution.

1. 0.05 M
2. 0.08 M
3. 1.00 M
4. 1.25 M

Q. The Molarity and molality of a given solution (solute + solvent) can be equal.

1. True
2. False