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Calculations with Acids and Bases

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I) Which one of these is the solute and which one is the solvent in a solution composed of i) 25.0 g of silver in 5.0 g of mercury, and ii) 3.0 g of iodine (I2) in 100.0 mL of ethanol?

ii) What is it that makes water such a good solvent for polar substances? Why is it called the universal solvent?

iii) What is the mass percent of a solution when 18.6 g of table salt is added to 81.4 g of water?

iv) Identify the electrolytes and the non-electrolytes among the following compounds:
(1) ethyl alcohol, C2H5OH
(2) potassium sulfate, K2SO4
(3) sodium bromide, NaBr
(4) methyl alcohol, CH3OH
(5) lithium chloride, LiCl

v) In a clean 250-mL volumetric flask, 125 mL of a 6.0 M hydrochloric acid was added. This was then diluted with more water to reach the 250-mL mark. What is the molarity of the acid at this time?

vi) Calculate the pH of 0.10 M HCl solution

vii) Calculate the final concentration if 4.0 L of 1.5 M NaCl and 2.0 L of 3.0 M NaCl are mixed.

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Solution Preview

i) Which one of these is the solute and which one is the solvent in a solution composed of i) 25.0 g of silver in 5.0 g of mercury, and ii) 3.0 g of iodine (I2) in 100.0 mL of ethanol?

Response: Solutes are substances that dissolve in solvents. Therefore, the silver is the solute while the mercury is the solvent, and the iodine is the solute and the ethanol is the solvent. Generally, the solute is the solid and the solvent is the liquid.

ii) What is it that makes water such a good solvent for polar substances? Why is it called the universal solvent?

Response: Water is great for dissolving polar substances because it is polar! Remember the ...

Solution Summary

This solution answers questions regarding solutes, solvents, mass percent, electrolytes/non-electrolytes, pH, and concentration.

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Solutions : Molarity; understanding acid-base titrations and balanced equations, C1V1=C2V2

I am confused on how to calculate the concentratin of the HCl solution -
below are the answers so far that I have to get the final answer -please help. I am stumped on question 2 The concentration of the NaOH is known to be 0.1M

1. For your most exact titration, record the following:

(a) Volume of NaOH solution in the burette at the start (mL): 50ml

(b) Volume of NaOH solution in the burette at the end (mL): 32 ml

(c) Volume of NaOH solution delivered to the flask (mL): 18 ml

(d) Volume of HCl solution in the flask (mL): 20 ml

2. Calculate the molarity of the HCl concentration from the equation:

C(acid) = C(base) * V(base) / V(acid)

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