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A 20.0 mL sample of 0.200 M HBr solution is titrated with 0.200 M NaOH solution. Calculate the pH of the solution after the following volumes of base have been added.
a) 14 mLb) 20.2 mL
An oxide of manganese consists of 77.4% manganese by mass. Determine its empirical formula and enter it in the box below.
Disscuss by IR spectrum and NMR. On my spectrum, it showed up 3282.57, 16557.91 and 16003.22. What are those wavelength are stand for
Write the Henderson-Hasselbalch equation for a solution of propanoic acid (CH3CH2CO2H, pKa = 4.874 ) using HA and A- in the expression. Using this equation, calculate the quotient [A-]/[HA] at A) pH 4.56 B) pH 4.874 C) pH 5.40.
Calculate the ratio of the translational partition functions of D2 and H2 at the same temperature and volume.
How many liters of dry carbon dioxide gas, measured at standard conditions will be evolved when 400 mL of a 0.20 M sulfuric acid are treated with an excess of potassium carbonate
1-hexanol was prepared by reacting an alkene with either hydroboration-oxidation or oxymercuration-reduction. Draw the structure of the alkene that was used to prepare the alcohol in highest yield.
A uniformly charged thin ring has radius 14.5cm and total charge 23.0nC . An electron is placed on the ring's axis a distance 30.0cm from the center of the ring and is constrained to stay on the axis of the ring. The electron is then released from..
The reaction of 0.25 g magnesium with 100 mL of 1 M hydrochloric acid (density d = 1.02 g/ml) raises the temperature of the solution from 20 °C to 35 °C . The specific heat for HCl is 3.93 J/(g.C).
A sample of 0.50 moles of O2 gas initially at 250K and a pressure of 1.0 atm is compressed to final pressure of 12 atm. The compression can occur via two different paths
A 3.84-mole sample of a gas is held at a temperature of 297 K and a pressure of 286 atm. Determine the volume of the gas sample.
Draw the structures of and label as the major and minor dehydrohalogenation products of reaction between 2-bromo-2-methylbutane with sodium ethoxide in ethanol.
Solubility of calcite (CaCO3) will increase with a decrease in temperature and decrease with an increase in temperature. This is because the solubility of calcite is dependent on the solubility of CO2.
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