Question 2 : How many moles of sulfate ions are in $200 mL$ of a $2 M$ sodium sulfate solution?

Question 3 : If $0.01$ mole of solute is present in $500\ ml $ of solution, its molarity is:

Question 4 : A 1.50 g sample of an ore containing silver was dissolved,and all the $ Ag^{+} $ was converted to 0.125 g $ Ag_{2}S $. What was the percentage of silver in the ore?

Question 7 : Stoichiometric ratio of sodium dihydrogen orthophosphate and sodium hydrogen orthophosphate required for synthesis of <img style='object-fit:contain' src="https://storage.googleapis.com/teachmint/question_assets/NEET/5ea7fed1a3d2442ab82937d8"> is

Question 9 : 0.52 g of dibasic acid required 100 mL of 0.1 <img style='object-fit:contain' src="https://storage.googleapis.com/teachmint/question_assets/NEET/5ea7fccdfdd8313cc8726705"> NaOH for complete neutralization. The equivalent weight of acid is:

Question 10 : Number of mole of 1 <img style='object-fit:contain' src="https://storage.googleapis.com/teachmint/question_assets/NEET/5ea7fe38fdd8313cc8726aac"> gas at NTP are:

Question 11 : The least count of an instrument is 0.01 cm. Taking all precautions, the most possible error in the measurement can be

Question 12 : If&#160;true enter $1$, else enter $0$.<br/>A decinormal solution is $\dfrac{1}{10}\ N$.

Question 13 : The number of moles of water in 488 g <img style='object-fit:contain' src="https://storage.googleapis.com/teachmint/question_assets/NEET/5ea7fdb5a3d2442ab829353d"> are:

Question 15 : The formula which represents the simple ratio of atoms in a compound is called:

Question 16 : The weight of&#160;${ H }_{ 2 }{ C }_{ 2 }{ O }_{ 4 }.2{ H }_{ 2 }O$ required to prepare&#160;500 ml of 0.2 N solution is:

Question 17 : Semimolar solution contains how many moles of solute in 1L of solution?

Question 19 : <b></b>Calculate the volume in 10 millimoles of solute present in&#160;0.08 M solution.

Question 20 : Which one of the following set of units represents the smallest and largest amount of energy respectively?

Question 21 : The weight, in grams, of KCl (Mol.wt. = 74.5) in&#160;100ml of a 0.1M KCl solution is:

Question 22 : Approximate atomic weight of an element is 26.89 . If its equivalent weight is 8.9 , the exact atomic weight of element would be :- -

Question 23 : A solution of known normality is diluted to two times. Which of the following changes during dilution?

Question 24 : The ratio of mole fraction of a solute and a solvent in a binary solution is:

Question 25 : The number of mole present in 2 litre of 0.5 <img style='object-fit:contain' src="https://storage.googleapis.com/teachmint/question_assets/NEET/5ea7fcdcfdd8313cc872674e"> NaOH is:

Question 26 : The molarity of a solution is 0.2 M when 18 g of glucose is dissolved in 500 ml of water.

Question 28 : Classify which of the following pair is a compound and a mixture?

Question 29 : A student performs a titration with different burettes and finds titre values of 25.2 mL, 25.25 mL, and 25.0mL. The number of significant figures in the average titre value is

Question 30 : The number of moles of solute present in 2.0 litre of 0.5 M NaOH solution is:

Question 31 : Five hundred milliliters of solution of 0.1 M $NaBr$ has how many milligrams of bromine?

Question 32 : For a solution of density, $d$ in g/ml containing&#160;solute of molecular weight $W$, the molarity $M$ and molality&#160;$m$&#160;are related by:

Question 34 : $200 \,ml$ of a solution contains $5.85 \,g$ dissolved sodium chloride. The concentration of the solution will be $(Na = 23 ; Cl = 35.5)$

Question 35 : What is the normality of a $1 \,M$ solution of $H_3PO_4$?

Question 36 : Calculate the molarity of each ion in solution after 2.0 litre of 3.0 M $AgNO_3$ is mixed with 3.0 litre of 1.0 M $BaCl_2$.

Question 37 : 200 ml of 0.25 M&#160;${ H }_{ 2 }{ SO }_{ 4 }$ is diluted to 250 ml. Normality&#160;of the solution becomes:

Question 38 : A current of $4.0A$ is passed for 5 hours through $1L$ of $2M$ solution of nickel nitrate using two nickel electrodes. The molarity of the solution at the end of the electrolysis will be:

Question 39 : $6.02\times 10^{20}$ molecules of urea are present in $100\ mL$ of its solution. The concentration of solution is:

Question 40 : The molarity of $4\ N\ H_2SO_4$ in the following reaction is $8H^+ +H_2SO_4 + 8e^- \to H_2S +4H_2O$

Question 41 : What is the mole fraction of glucose in $10\%\ w/W$ glucose solution?

Question 42 : If 5.85 g of NaCl (molecular weight 58.5) is dissolved in water and the solution is made up to 0.5 litre, the molarity of the solution will be

Question 43 : Choose the correct statement:<div><br/>i) Normality and molarity of HCl are same.</div><div><br/>ii) Molality and molarity are independent of temperature.</div><div><br/>iii) Normality of 1M&#160;${ KMnO }_{ 4 }$ in acidic medium&#160;is 5 N.</div>

Question 44 : For preparing $0.1\ N$ solution of a compound from its impure sample of which the percentage purity is known, the weight of the substance required will be :

Question 45 : Calculate&#160;the value of $100\ x$ if $x$ mL is the volume of water required to make $1\ \text N$ solution from $2$ mL concentration $HNO_3$.<br/>

Question 47 : A 5 molar solution of ${ H }_{ 2 }S{ O }_{ 4 }$ is diluted form $1 L$ to $10 L$. What is the normality of the solution?

Question 48 : The expression relating mole fraction of solute ($x_2$) and molarity ($M$) of the solution is:

Question 49 : 10 millimoles of a di-acidic base exactly neutralize 100 ml&#160;of acid. Then, the normality of that acid is:

Question 50 : A container when is empty weights $50 gm$. After certain of density ${ 25 gm/dm }^{ 3 }$ is filled its mass becomes equal to $100 gm$. The volume of the container will be:

Question 51 : A solution contain $36\%$ water and $64\%$ acetaldehyde $(CH_2CHO)$ by mass. The mole fraction of acetaldehyde is:

Question 52 : $35.4\ mL$ of $HCl$ is required for the neutralization of a solution containing $0.275\ g$ sodium hydroxide. The molarity of hydrochloric acid is:

Question 53 : The ammonia evolved from the treatment of $0.30\ g$ of an organic compound for the estimation of nitrogen was passed in $100\ mL$ of $0.1\ M$ sulphuric acid. The excess of acid required $20\ mL$ of $0.5\ $ sodium hydroxide solution hydroxide solution for complete neutralization. The organic compound is:

Question 54 : At NTP, 1 L of $O_2$ reacts with 3 L of carbon monoxide. What will be the volume of CO and $CO_2$ after the reaction?

Question 55 : What is the molarity of $H_{2}SO_{4}$ solution present initially in the container?

Question 56 : $5$ ml of $1N$&#160;HCl, $20$ ml of $\dfrac{N}{2}$ $H_2SO_4$ and $30$ ml of $\dfrac{N}{3}$ $HNO_3$ are mixed together and the volume is made to $1$ L. The normality of the resulting solution is&#160;:

Question 57 : The density of a $3 \,M$ sodium thiosulphate $(Na_2S_2O_3)$ solution is $1.25 \,gm/ml$. Calculate the percentage by weight of sodium thiosulphate.

Question 58 : 1 mole of the substance present is 1 L of solution is known as:

Question 60 : &#160;$4.0 g$&#160; of&#160; $NaOH$&#160; is dissolved in&#160; $100\mathrm { cc }$&#160; of solution. The normality of the solution is:

Question 61 : The volume inline liters of $CO_{2}$ liberated at $STP$ when $10g$ of $90\%$ pure limestone is heated completely is:<br/>

Question 62 : Calculate the molarity of a solution containing 20.7 g of potassium carbonate dissolved in 500 mL of solution (assume density of solution = 1 g mL$^{-1}$).

Question 63 : Strength in volumes of a solution containing $30.36\ g/litre$ of $H_2O_2$ is:&#160;

Question 64 : What mass of sodium carbonate, $Na_2CO_3$&#160; is needed to make 120 mL of a 1.5 M solution? (Given formula weight of sodium carbonate = 106 amu)

Question 66 : Assertion: Greater the mole fraction of a gas in gaseous mixture, greater is the pressure it exerts. Reason: Pressure of gas is due to bombardment of gas molecules on the walls of the container.

Question 67 : In an auto engine with no pollution controls, about 5% of the fuel $(C_{8}H_{18})$&#160;is unburned. Molar ratio of $CO$ and $(C_{8}H_{18})$, emitted in the exhaust gas is:

Question 71 : Determine the molarity of solution obtained by mixing $50ml$ of $0.26M\ H_{2}SO_{4}$ solution with another $150ml$ of $0.48M\ H_{2}SO_{4}$ solution?

Question 72 : $\displaystyle 2N$&#160;$\displaystyle HCl$ solution will have same molar concentration as a:

Question 73 : Volume of $0.1M$ oxalic acid, which can completely decolourise $20 ml$ of $0.1M \ KMnO_{4}$ in acidic medium, is:

Question 74 : Normality of 1% ${ H }_{ 2 }{ SO }_{ 4 }$ solution is nearly:<br>

Question 76 : What is the molarity of 25% of (w/v) solution of HCI?

Question 77 : If 98 grams of $\displaystyle { H }_{ 2 }{ SO }_{ 4 }$ is added in sufficient water to make 500 milliliters of solution, then what is the molarity of a solution?

Question 78 : Concentrated sulphuric acid has density of 1.9 g/mL and $99\%$ $H_2SO_4$ by mass. Calculate the molarity of the acid.

Question 79 : $NaClO$ solution reacts with $H_{2} S_{4}O$. Solution of $NaClO$ used in the reaction&#160;contained 15g of NaClO per litre.&#160;The normality of the solution would be:

Question 80 : What is the molarity of $HCl$ in a solution prepared by dissolving 5.5 g $HCl$ in 200 g ethanol if the density of the solution is 0.79 g/ mL?<br/>

Question 81 : The weight percent of source (formula weight &#160;= 342 $g\ mol^{-1} $ ) in an aqueous solution is 3.42. The density of the solution is 1 $g\ mL^{-1} $ , the concentration of sucrose in the solution in $ mol \ L^{-1} $ is:&#160;

Question 83 : $1$ mole $N_{2}$ and $4$ mole $H_{2}$ are allowed to react in a vessel and after reaction $H_{2}O$ is added to the vessel. Aqueous solution required $1$ mole $HCl$. Mole fraction of $H_{2}$ in the gaseous mixture after the reaction is:

Question 84 : $5.5\ mg$ of nitrogen gas dissolves in $180\ g$ of water at $273\ K$ and one atm pressure due to nitrogen gas. The mole fraction of nitrogen in $180\ g$ of water at $5\ atm$ nitrogen pressure is approximately :

Question 85 : A candle is burnt in a beaker until it extinguishes itself. A sample of gaseous mixture in the beaker contains $6.08\times 10^{20}$ molecules of $N_2, 0.76\times 10^{20}$ molecules of $O_2$, and $0.50\times 10^{20}$ molecules of $CO_2$. The total pressure is 734 mm of Hg. The partial pressure of $O_2$ would be:

Question 87 : What $\%$ of the carbon in the $H_2CO_3-HCO^-_3$ buffer should be in the form of $HCO^-_3$ so as to have a neutral solution? $(K_a=4\times 10^{-7})$

Question 88 : Consider the following solutions,<div><br/>(a) $4$ g of caustic soda is dissolved in $200$ mL of the solution.<br/>(b) $5.3$ g of anhydrous sodium carbonate is dissolved in $100$ mL of solution.<br/>(c) $0.365$ g of pure HCl gas is dissolved in $50$ mL of solution.</div><div><br/>The&#160;molarity of these solutions respectively are :<br/></div>

Question 89 : An aqueous solution of concentrated hydrobromic acid contains $48\%$ $HBr$ by mass. If the density of the solution is $1.50$ g/mL, what is its concentration?<br>

Question 90 : To a 25 ml $ H_{2}O_{2}$ solution, excess of acidified solution of potassium iodide was added. The iodine liberated required 20 ml of $ 0.3 N \ Na_{2}S_{2}O_{3}$ solution. The volume strength of $ H_{2}O_{2}$ solution is:

Question 92 : If $200$ml solution of $0.5$M $NaOH$ is diluted to $800$ml then find molarity of resultant solution.

Question 93 : A $5.0$ mL solution of $H_{2}O_{2}$ liberates $0.508$ g of iodine from an acidified $KI$ solution. The strength of&#160;$H_{2}O_{2}$&#160;solution in terms of&#160;volume strength at $STP$ will be :

Question 95 : 100 ml of 10V $H_2O_2$ solution is heated. The evolved gas is completely reacted with Ca to form CaO. The aqueous solution of Cao is neutralised by 50 ml of $H_2SO_4$ solution. The molarity of $H_2SO4$ is:

Question 96 : A 3.4 g sample of H$_2$O$_2$ solution containing $x\%$ H$_2$O$_2$ by mass requires x ml of a KMnO$_4$ solution for complete oxidation under acidic condition. The molarity of KMnO$_4$ solution is :

Question 97 : Match the List - I with List - II and pick up the correct matching from the codes given below:<br/><table class="wysiwyg-table"><tbody><tr><td>List - I<br/>(Electrochemical Parameter)</td><td>List - II<br/>(Units)</td></tr><tr><td>(I) Ionic mobility</td><td>1. $cm^{-1}$</td></tr><tr><td>(II) &#160;Cell constant</td><td>2. $ohm^{-1}\, cm^{-1}$</td></tr><tr><td>(III) Specif conductance&#160;</td><td>3. $ohm^{-1}\, cm^{-1}\, mol^{-1}$</td></tr><tr><td>(IV) Molar conductance&#160;</td><td>4. $cm^2\, V^{-1}s^{-1}$</td></tr><tr><td><br/></td><td><br/></td></tr></tbody></table>

Question 98 : A solution of $KMnO_4$ containing $3$ g/L is titrated with a solution of $H_2O_2$ containing $2$ g/L.<div>The volume (in ml)&#160;of $KMnO_4$ required to react with $20$ mL $H_2O_2$ solution is: (as nearest integer)&#160;</div>

Question 99 : $300$ g of an aqueous solution of a particular solute (containing $30$%&#160;solute&#160;by mass) is mixed with $400$ g of another&#160;aqueous&#160;solution of the&#160;same&#160;solute (containing $40$% solute by mass).&#160;In the final solution, mass $\%$ of solute is :<div>[Given, Molecular mass of solute $\displaystyle = 50$]<br/></div>

Question 100 : The molarity of a solution in which $5.3$g $Na_2CO_3$ is dissolved in $500$ mL will be:

Question 101 : What molar concentration of $NH_3$ provides a $[OH^-]$ of $1.5 \times 10^{-3}$ ?<br>$(K_b = 1.8 \times 10^{-5})$

Question 102 : Sulphuric acid reacts with sodium hydroxide as follows&#160;<br/>$H_2SO_4$ + $2NaOH$ $\rightarrow$ $Na_2SO_4$+ $2H_2O $<br/>When 1 L of 0.1 M sulphuric acid solution is allowed to react with 1 L of 0.1 M sodium hydroxide solution, the amount of sodium sulphate formed and its molarity in the solution obtained is ?

Question 103 : Gaseous ${N}_{2}{O}_{4}$ dissociates into gaseous ${NO}_{2}$ according to the reaction ${N}_{2}{O}_{4}(g)\rightleftharpoons 2{NO}_{2}(g)$. At $300K$ and $1atm$ pressure, the degree of dissociation of ${N}_{2}{O}_{4}$ is $0.2$. If one mole of ${N}_{2}{O}_{4}$ gas is contained in a vessel, then the density of the equilibrium mixture is:

Question 104 : From the following data of $\Delta H$, of the following reactions,<div><br/>$C(s)+\dfrac{1}{2}O_2(g)\rightarrow CO(g)AH=-110$ kJ<br/>$C(s)+H_2O(g)\rightarrow CO(g)+H_2(g)\Delta H=132$ kJ</div><div><br/>What is the mole composition of the mixture of steam and oxygen on being passed over a coke at $1273$ K, keeping the temperature constant?<br/></div>

Question 105 : The volume of $0.05 \,M H_{2}SO_{4}$ required to neutralise $80 \,ml $ of $0.13 \,N \,NaOH$ will be

Question 106 : If 25 mL of a $H_2SO_4$ solution reacts completely with 1.06 g of pure $Na_2CO_3$, what is the normality of this acid solution?

Question 107 : Molarity of solution containing $12.6$ grams of oxalic acid in $100\ ml$ of the solution is:&#160;

Question 108 : Potassium permanganate acts as an oxidising agent in acidic, alkaline as well as neutral media. Which among the following statements is incorrect?

Question 109 : Molarity of $Ca_{3}(PO_{4})_{2}$ if the molarity of the calcium ions in the same solution is $3M$:

Question 110 : Two oleum samples $A$ and $B$ have labeling $109%$ and $118%$ respectively. $100\ g$ of $A$ is diluted to an a $1\ L$ solution and $100\ g$ of $B$ is diluted to a $1000\ mL$ solution. If both these solutions are mixed, then normality of $H_{2}SO_{4}$ (approx.) in final solution is:

Question 111 : In an ideal mixture of liquid A and B the mole fraction of A is 0.25 . If the ratio of $ P^0_A $ to $ P^0_B $ is 7/3. how many repeated distillations would be required as a minimum to obtain a small quantity of distillate which has a mole fraction of A , better than 0.80 ?

Question 112 : A $15$ mL sample of $0.20\ M\ MgCl_2$ is added to $45$ mL of $0.40\ M\ AlCl_3$, what is the molarity of $Cl^{-}$ions in the final solution?

Question 113 : What is the normality of 0.3 M $ H_3PO_4 $ when it undergoes the reaction?<div><br/><div>$ H_3PO_4 +20H^- \rightarrow HPO^{2-}_3 +2H_2O $</div></div>

Question 114 : $500$&#160;g of urea solution of mole fraction&#160;$0.2$&#160;is diluted to&#160;$1500$&#160;g. The mole fraction of&#160;solute&#160;in&#160;the diluted solution is:

Question 116 : <u></u>If $500mL$ of a $5M$ solution is diluted to $1500mL$, the molarity of the dilute solution is:

Question 117 : A mixture of $Na_2C_2O_4$ ($A$) and $KH_2C_2O_4.2H_2O$ ($B$) required equal volumes of $0.1$ M $KMnO_4$ and $0.1$ M $NaOH$ separately. Molar ratio of $A$ and $B$ in the mixture is&#160;:

Question 118 : What is the mole fraction of the solute in a $1.00$ m aqueous solution?

Question 119 : The molarity of solution and weight of sodium bromate necessary to prepare $85.5$ mL of $0.672\: N$ solution when the half-cell reaction is $BrO^{\circleddash}_3 + 6H^{\bigoplus}+ 6e^-\rightarrow Br^{\circleddash} + 3H_2O$, are respectively :