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The following questions refer to a 2.0-liter buffered solution created from 0.500 NH3 (kb=1.8 x 1-^-5) and 0.250 M NH4Cl. Q1 Calculate the pH of this solution? Q2 When 0.100 mol of H+ ions is added to the solution what is the pH (assuming volume did not change)?
Calculate the molar mass of the uknown compound. The boiling point elevation constant for water is0.52°C/m
What is the molality of chromium(III) chloride in a solution prepared by dissolving 75.2 g chromium(III) chloride hexahydrate (CrCl3· 6H2O) in 250.0 g of water.
When an acid or a base is added to a buffer, a double-displacement reaction will occur. The acid or base will be neutralized, forming a neutral salt or water plus the conjugate of the buffer.
Calculate the pH of a solution formed by mixing 250 mL of 0.150 M NaHCO3 with 250 mL of 0.100 M Na2CO3. What is the molarity of the prepared buffer?
What is the predominant form of Ile at pH 6 (assuming the pKa of the carboxylate is 3 and the amino group is 9?
Calculate the inital pH of buffers A, B, & C using the Henderson-Hasselbach equation.
What is the freezing point of a solution prepared by dissolving 11.3g of Ca(NO3)2 in 115g of water? (The molal freezing point depression of constant water is 1.86 °C/m).
How many milliliters of 0.459 M HBrO4 are needed to titrate each of the following solutions to the equivalence point. (a) 21.2 mL of 0.505 M KOH mL (b) 30.7 mL of 0.551 M NaOH mL
the reaction of copper(I) sulfide with oxygen gas as follows: Cu2(s) + O2(g) ? 2Cu(s) + SO2(g) If 0.330 kg of copper(I) sulfide reacts with excess oxygen, what mass of copper metal may be produced
Calculate the pH and pOH of the solutions with the following hydrogen ion or hydroxide ion concentrations. Indicate which solutions are acidic, basic, or neutral
What is the concentration of a solution made by diluting 75 mL of 6.0 M HCl to a final volume
Which of the following pairs of substances are miscible and which are not?
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