Question 1 :
If true enter $1$, else enter $0$.<br/>A decinormal solution is $\dfrac{1}{10}\ N$.
Question 2 :
The least count of an instrument is 0.01 cm. Taking all precautions, the most possible error in the measurement can be
Question 4 : 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 5 :
<b></b>Calculate the volume in 10 millimoles of solute present in 0.08 M solution.
Question 6 :
The number of moles of solute present in 2.0 litre of 0.5 M NaOH solution is:
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 :
The weight of ${ H }_{ 2 }{ C }_{ 2 }{ O }_{ 4 }.2{ H }_{ 2 }O$ required to prepare 500 ml of 0.2 N solution is:
Question 10 :
The formula which represents the simple ratio of atoms in a compound is called:
Question 11 :
How many moles of sulfate ions are in $200 mL$ of a $2 M$ sodium sulfate solution?
Question 12 :
The molarity of a solution is 0.2 M when 18 g of glucose is dissolved in 500 ml of water.
Question 15 :
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 16 :
A solution of known normality is diluted to two times. Which of the following changes during dilution?
Question 18 :
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 19 :
Semimolar solution contains how many moles of solute in 1L of solution?
Question 21 : 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 22 : 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 24 :
Classify which of the following pair is a compound and a mixture?
Question 25 :
The ratio of mole fraction of a solute and a solvent in a binary solution is:
Question 26 :
10.6 g of a substance of molecular weight 106 was dissolved in 100 ml. 10 ml of this solution was pipetted out into a 1000 ml flask and made up to the mark with distilled water. The molarity of the resulting solution is:<br/>
Question 27 :
Volume of 0.1M ${ H }_{ 2 }{ SO }_{ 4 }$ is required to neutralise 50ml of 0.2M NaOH solution is:
Question 28 :
If $30$ mL of $0.5$ M $H_2SO_4$ diluted to $500$ mL $H_2SO_4$, then what will be it's molarity?
Question 29 :
The volume inline liters of $CO_{2}$ liberated at $STP$ when $10g$ of $90\%$ pure limestone is heated completely is:<br/>
Question 30 :
Equal volumes of $0.1\ M$ $AgN{O}_{3}$ and $0.2\ M$ $NaCl$ are mixed. The concentration of $N{O}_{3}^{-}$ ion in the mixture will be :
Question 32 :
The expression relating mole fraction of solute ($x_2$) and molarity ($M$) of the solution is:
Question 33 :
Five hundred milliliters of solution of 0.1 M $NaBr$ has how many milligrams of bromine?
Question 34 :
The mole fraction of A in 10% (w/w) aq. solution of glucose is:
Question 35 :
$2.5$ litre of $1\ M\ NaOH$ solution mixed with another $3$ litre of $0.5\ M\ NaOH$ solution. Then find out molarity of resultant solution.
Question 37 :
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 38 :
For a solution of volatile liquids the partial vapour pressure of each component in solution is directly proportional to
Question 39 :
2.46 g of sodium hydroxide (molar mass = 40) are dissolved in water and the solution is made to 100 $cm^3$ in a volumetric flask. Calculate the molarity of the solution.
Question 40 :
What is the molarity of 25% of (w/v) solution of HCI?
Question 41 :
The ${P}^{H}$ of a dibasic acid is $3.699$. Its molarity is?
Question 42 :
If 6 M $KOH$ solution is 28% by weight, then what is the specific gravity of this solution?
Question 43 :
How much water, in litres, must be added to $0.5 L$ of $6 M$ $HCl$ to make it $2 M$?
Question 44 :
The molarity of 15% (w/w) solution of ${ H }_{ 2 }{ SO }_{ 4 }$ of density 1.1 g/cc is:
Question 45 :
If the concentration of glucose $(C_6 H_{12} O_6)$ in blood $0.9\ g\ L^{-1}$, what will be the molarity of glocose in blood?
Question 46 :
Normality of 1% ${ H }_{ 2 }{ SO }_{ 4 }$ solution is nearly:<br>
Question 48 :
A gas mixture of $3$ liters of propane and butane on complete combustion at $25^{o}C$ produced $10$ liters of $CO_{2}$ initial composition of the propane & butane in the gas mixture is:<br/>
Question 49 :
$3.01\times 10^{23}$ molecules of elemental Sulphur will react with 0.5 mole of oxygen gas completely to produce<br>
Question 50 :
 $4.0 g$  of  $NaOH$  is dissolved in  $100\mathrm { cc }$  of solution. The normality of the solution is:
Question 51 :
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 52 :
<u></u>If $500mL$ of a $5M$ solution is diluted to $1500mL$, the molarity of the dilute solution is:
Question 53 :
$5.5\ mg$ 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 54 :
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 55 :
The molarity of a solution in which $5.3$g $Na_2CO_3$ is dissolved in $500$ mL will be:
Question 56 :
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 :
Question 59 :
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 60 : 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) of $KMnO_4$ required to react with $20$ mL $H_2O_2$ solution is: (as nearest integer) </div>
Question 61 : 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 63 :
Molarity of $Ca_{3}(PO_{4})_{2}$ if the molarity of the calcium ions in the same solution is $3M$:
Question 64 : $300$ g of an aqueous solution of a particular solute (containing $30$% solute by mass) is mixed with $400$ g of another aqueous solution of the same solute (containing $40$% solute by mass). In the final solution, mass $\%$ of solute is :<div>[Given, Molecular mass of solute $\displaystyle = 50$]<br/></div>
Question 65 :
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 66 : 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 67 :
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 68 :
Sulphuric acid reacts with sodium hydroxide as follows <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 69 :
$500$ g of urea solution of mole fraction $0.2$ is diluted to $1500$ g. The mole fraction of solute in the diluted solution is:
Question 71 :
$1$ 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 72 :
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 73 :
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 74 :
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 75 :
What molar concentration of $NH_3$ provides a $[OH^-]$ of $1.5 \times 10^{-3}$ ?<br>$(K_b = 1.8 \times 10^{-5})$
