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Using Tables from the book when needed, determine the pH at the equivalence point in the titration of 28.5 mL of 0.694 M pyridine, C6H5N, by 0.770 M HNO3.
Calculate the molarity of each of the following solutions(a) 29.0 g of ethanol (C2H5OH) in 545 mL of solution.
A tablet of Vitamin C changed color at 23.7 mLs of Iodine. how do you determine how much vitamin c is in the tablet.
Find out the Celsius temperature of 2.49 mol of gas contained in a 1.00 L vessel at 1.8 atm pressure.
A stock solution is prepared by adding 24 mL of 0.4 M Na3PO4 to enough water to make 79 mL. What is the PO43- concentration of 25 mL of the stock solution?
how many moles of CO2 are produced when 5.40 mol of ethane are burned in an excess of oxygen
Consider the cell prepared with 2.0 M Cd2+ and 0.45 M Zn2+ solutions: Zn(s) + Cd2+(aq) --- Zn2+(aq) + Cd(s)
Ice cream mix containing 40% total solids is frozen so that half of the original water is made into ice (which is effectively pure water). If the mix contained 12% fat, 16% sugar, and 12% nonfat milk solids
A 5.0 L sealed bottle containing 0.26 g of liquid ethanol, C2H6O, is placed in a refrigerator and reaches equilibrium with its vapor at -11°C. The vapor pressure of ethanol is 10 torr at -2.3°C and 40 torr at 19°C.
Calculate the concentrations of all species at equilibrium for the following case.
total molarity of acid and conjugate base in this buffer. A boy mixes 5.70mL of a 0.330M Hydrochloric acid solution to the beaker. Determine the pH change if The pKa of acetic acid = 4.760.
suppose you wanted to dissolve 106 g of Na2CO3 in enough H2O to make 6.00L of solution what is the molar mass of Na2CO3.
What is the molar concentration of a solution prepared by dissolving 0.6593 g of NaCl in a 100-mL volumetric flask
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