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A student was as ked to determine the molecular weight of a weak monoprotic dry acid (HX). She was provided the following laboratory equipment: a balance (accurate to 0.001g), distilled water, a 100.00 mL volumetric flask, a supply of sodium hydroxide solution of unknown concentration, a bottle of phenolphthalein, a 100.00 mL graduated cylinder (accurate to 0.01 mL), and a supply of oxalic dihydrate (H2C2O4. 2H2O).
Suppose the student had used 20.00 grams of the acid and dissolved the acid in distilled water to bring the volume to exactly 100.00 mL. She then added several drops of phenolphthalein to the acidic solution. She then titrated a 50.00 mL sample of this acidic solution with the sodium hydroxide solution and found that it took 42.33 mL of NaOH to reach the end point. She repeated her procedure and found that it took 42.89 mL of NaOH to reach the end point. In order to determine the molarity of the sodium hydroxide solution, she discovered that it took exactly 50.00 mL of sodium hydroxide solution to neutralize 1.500 grams of oxalic acid dihydrate.
i. Determine the molarity of the NaOH solution.ii. Calculate the molecular weight of the unknown acid.
Organic chemists rely heavily on the spectroscopic methods of IR and NMR. Explain in great detail (that means more than 2 or 3 sentences) why the two methods have to be used in tandem to determine
A direct current was passed through a solution containing alanine, Match the behavior with correct amino acid. The isoelectric point of histidine is 10.0.
How many liters of hydrogen gas are collected over water at 18 degrees Celsius and 725 mmHg when 0.84 g of lithium reacts with water?
To verify Boyle's Law using the relationship between gas volume and gas pressure when the amount of gas remains constant at certain temperature.
Calculate the pH after 15.0 mL of 0.40M HCL is added to 20.0 mL of 0.50 M NH3 (Kb NH3= 1.8 x 10^-5)
Determine the oxidation number for the indicated element in each of the following substances.
A 0.0100 molal aqueous solution of a weak acid freezes at -0.0205 oC. Calculate the percent ionization of the weak acid, HA.
Silver has an average atomic mass of 107.87 u. If 48.18% of Ag exists as Ag-109 (108.9047 u), what is the identity and the atomic mass of the other isotope?
What is the name of the compound (NH4)3PO3? Why is special about this compound? Choose one answer. a. Ammonium phosphate; this covalent compound is made up of two polyatomic ions, ammonium and phosphate.
A mixture of Ar and N2 gases has a density of 1.416 at STP. What is the mole fraction of each gas?
How many additional mL of 0.0750 M Ca(OH)2 or ).100 M HCl would be required to neutralize the solution?
A saturated solution of calcium iodate, Ca(IO3)2, is created by suspending a small amount of pure solid of Ca(IO3)2 in 50.0 mL of distilled water.
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