Question 1 :
Which one of the following set of units represents the smallest and largest amount of energy respectively?

Question 2 :
If&#160;true enter $1$, else enter $0$.<br/>A decinormal solution is $\dfrac{1}{10}\ N$.

Question 3 :
<b></b>Calculate the volume in 10 millimoles of solute present in&#160;0.08 M solution.

Question 7 :
Classify which of the following pair is a compound and a mixture?

Question 8 :
The number of moles of solute present in 2.0 litre of 0.5 M NaOH solution is:

Question 9 :
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 11 :
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 12 :
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 14 :
The ratio of mole fraction of a solute and a solvent in a binary solution is:

Question 15 :
Semimolar solution contains how many moles of solute in 1L of solution?

Question 16 :
How many moles of sulfate ions are in $200 mL$ of a $2 M$ sodium sulfate solution?

Question 17 :
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 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 :
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 20 :
The molarity of a solution is 0.2 M when 18 g of glucose is dissolved in 500 ml of water.

Question 21 :
The molarity of $4\ N\ H_2SO_4$ in the following reaction is $8H^+ +H_2SO_4 + 8e^- \to H_2S +4H_2O$

Question 22 :
The expression relating mole fraction of solute ($x_2$) and molarity ($M$) of the solution is:

Question 23 :
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 24 :
A sulphuric acid solution contains $98\%$ $(m/v)H_{2}SO_{4}$. The density of the solutions is $1.98 \ gcm^{3}$. The molarity and molatity respectively of the solution are:

Question 25 :
A solution is made by dissolving $49\ g$ of $H_2SO_4$ in $250\ mL$ of water. The molarity of solution prepared is:

Question 26 :
<u></u>If $500mL$ of a $5M$ solution is diluted to $1500mL$, the molarity of the dilute solution is:

Question 27 :
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 28 :
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>