Questions in solutions

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	The formula weight of ${{H}_{2}}S{{O}_{4}}$ is 98. The weight of the acid in $400ml$ of $0.1M$ solution is
	$25ml$ of $3.0M\ HN{{O}_{3}}$ are mixed with $75ml$ of $4.0M\ HN{{O}_{3}}$. If the volumes are additive, the molarity of the final mixture would be
	How many grams of HCl will be present in 150 ml of its 0.52 M solution
	How many litres of $C{{O}_{2}}$ at STP will be formed when $100ml$ of $0.1M\ {{H}_{2}}S{{O}_{4}}$ reacts with excess of $N{{a}_{2}}C{{O}_{3}}$
	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 upto the mark with distilled water. The molarity of the resulting solution is
	A certain aqueous solution of $FeC{{l}_{3}}$(formula mass =162) has a density of $1.1\,g/ml$and contains 20.0% $FeC{{l}_{3}}.$Molar concentration of this solution is
	If 0.50 mole of $CaC{{l}_{2}}$is mixed with 0.20 mol of $N{{a}_{3}}P{{O}_{4}},$the maximum number of moles of $C{{a}_{3}}{{(P{{O}_{4}})}_{2}}$which can be formed, is
	25 ml of a solution of barium hydroxide on titration with a 0.1 molar solution of hydrochloric acid gave a litre value of 35 ml. The molarity of barium hydroxide solution was
	2.5 litre of 1M NaOH solution are mixed with another 3 litre of 0.5 M NaOH solution. Then the molarity of the resulting solution is
	The molar solution of sulphuric acid is equal to