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You are provided with 10ml of 0.10M stock solution of NaOH. Describe how you would prepare 0.02M solution from the stock solution
A compound has an empirical formula of C7H12O and a formula mass of 224 g/mol. What is the compound’s molecular formula?
1.3 An open-end mercury manometer was connected to a flask containing a gas at unknown pressure. The mercury in the arm open to the atmospheric pressure was 76mm lower than the mercury in the arm connected to the flask. The atmospheric pressure 749 torr. What was the Pressure of the gas in the flask in Pascal
How many moles of gas are there in a sample occupying 1.74 L at 0.136 atm and 25°C?
25.00 mL of an aqueous 0.10 M CaCO3 solution is titrated with a 0.20 M HCl solution at room temperature, using methyl orange as the indicator. The color of the solution changed from the initial yellow color to a shade of orange when 23.15 mL of the titrand was added.
a). Using the above titration result, explain the difference between the endpoint and equivalence point for a titration.
b). Aqueous solutions of CaCO3 are considered as primary standards while HCl solutions can be used only as secondary standards. Briefly explain why.
What will be the volume of HCl required for the above titration if phenolphthalein was used as the indicator? Write balanced chemical equations for the titration
If n A of current pass for 2 minutes at the cathode where a group I ion X+ dissociates 0.4moles of A reacts with dil H2SO4 and (n2/2)g of a salt (B) is produced. What quantity of charge was deposited at the cathode (RMM of B=2n)?
Why does an atom of aluminium form ion while that of carbon does not ?
A sample of concentrated HCl solution with 88% by mass and density of 1.43 g cm⁻³. Calculate the molality of the solution
If one mole of Na contains x atoms of sodium, what is the number of moles contained in 46g of sodium?
