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1 M, 2.5 litre NaOH solution is mixed with another 0.5 M and 3 litre NaOH solution. The molarity of the resultant solution will be:
An organic compound contains 80 % (by wt.) carbon and the remaining percentage of hydrogen. The empirical formula of this compound is: [Atomic wt. of C is 12, H is 1]
Calculate the mass of 95% pure $CaCO_3$ that will be required to neutralize 50 mL of 0.5 M HCl solution according to the following reaction: $$ CaCO_3(s) + 2HCl(aq) \rightarrow CaCl_2(aq) + CO_2(g) + 2H_2O(l) $$ [Calculate up to the second place of decimal point]
Match List-I with List-II: | List-I (Quantities) | List-II (Corresponding Values) | | :--- | :--- | | (a) 4.48 litres of $O_2$ at STP | (i) 0.2 mole | | (b) $12.022 \times 10^{22}$ molecules of $H_2O$ | (ii) $12.044 \times 10^{23}$ molecules | | (c) 96 g of $O_2$ | (iii) 6.4 g | | (d) 88 g of $CO_2$ | (iv) 67.2 litres at STP | (Given - Molar volume of a gas at STP = 22.4 L)
The density of a $2 \text{ M}$ aqueous solution of $NaOH$ is $1.28 \text{ g/cm}^3$. The molality of the solution is: [molecular mass of $NaOH = 40 \text{ g mol}^{-1}$]
Among the following, isoelectronic species are:
A compound X contains 32% of A, 20% of B and remaining percentage of C. Then, the empirical formula of X is: (Given atomic mass of A = 64; B = 40; C = 32 u)
Which of the following contains the highest number of helium atoms?
A 1 M solution of a compound 'X' has a density of 1.25 g/mL. If the molar mass of compound X is 85 g, what is the molality (m) of the solution?
The molar mass of a compound (X), whose $2.6 \text{ mol}$ weighs $312 \text{ g}$, is:
Which of the following contains the maximum number of atoms?
How many moles of lead (II) chloride will be formed from a reaction between $6.5\text{ g}$ of $\text{PbO}$ and $3.2\text{ g}$ of $\text{HCl}$?
The number of water molecules is maximum in:
When $50\text{ mL}$ of a $16.9\%\text{ (w/v)}$ solution of $\text{AgNO}_3$ is mixed with $50\text{ mL}$ of $5.8\%\text{ (w/v) NaCl}$ solution, then the mass of precipitate formed is: ($\text{Ag} = 107.8$, $\text{N} = 14$, $\text{O} = 16$, $\text{Na} = 23$, $\text{Cl} = 35.5$)
$10\text{ g}$ of hydrogen and $64\text{ g}$ of oxygen were filled in a steel vessel and exploded. The amount of water produced in this reaction will be:
The number of atoms in $0.1\text{ mole}$ of a triatomic gas is: ($N_A = 6.02 \times 10^{23}\text{ mol}^{-1}$)
Match List-I (Molecules) with List-II (Shapes): List-I: (a) $PCl_5$ (b) $SF_6$ (c) $BrF_5$ (d) $BF_3$ List-II: (i) Square pyramidal (ii) Trigonal planar (iii) Octahedral (iv) Trigonal bipyramidal Choose the correct answer from the options given below:
Calculate the mole fraction of the solute in a $1.00 \text{ m}$ aqueous solution.
The volume of oxygen gas ($\text{O}_2$) needed to completely burn $1 \text{ L}$ of propane gas ($\text{C}_3\text{H}_8$) (both $\text{O}_2$ & propane measured at $0^\circ\text{C}$ and $1 \text{ atm}$) will be:
A magnetic moment of 1.73 BM will be shown by one among the following: