Hydrogen and chlorine gas are placed in a 10.0 L container and allowed to react. The...

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Chemistry

Hydrogen and chlorine gas are placed in a 10.0 L container andallowed to react. The initial density of the mixture is 5.01 x10-3gm/ml. The vessel is at 300K and the initial pressure is 6.52 atm.After the reaction is complete , the pressure is 6.52 atm. The gasis bubbled into 1.00 liter of deionized water. In another part ofthe universe, a grey haired chemistry instructor prepares an aceticacid/ acetate buffer. The buffer was prepared by adding acetic acidand sodium acetate to 2.50 L of deionized water. Now, as universescollide, our hero adds 107 ml of the HCl solution to 405 ml of thebuffer. The pH is measured and is 4.35 after the HCl addition. Adrop of phenolphthalein is added and the solution is titrated toequivalence with 657 ml of 0.920 M NaOH. Calculate the originalmolarities of the weak acid and conjugate base in the 2.50 Lsolution?

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4.2 Ratings (855 Votes)

Let us start by writing out the equations one by one H2 Cl2 2HCl We assume ideal gas behaviour to obtain the moles of HCl produced We have the following parameters supplied P 652 atm V 100 L T 300 K Using the ideal gas law we have 652 atm100 L nR300 K w here n amount of the ideal gas in moles and R universal gas constant having a value of 0082 LatmmolK Putting the values we obtain n 652 atm100 L0082 LatmmolK300 K or n 26504 mole Now 26504 mole HCl is dissolved in 10 L water so the molarity of the resulting solution is 26504 mol1 L 26504 M Now we move to the other part of the problem Let the original solution contain x mole of acetic acid and y mole of sodium acetate buffer so that the molarity of the See Answer

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