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A 25.00mL 0.200 M HCL solution is titrated with 0.2 M NaOH. Explain what is the pH after the addition of 10.00mL of NaOH?
1.07
12.9
0.9
8.5
2.85
Discuss the trend in ion size within a family and a period and put a group of ions in order of increasing (decreasing) ion size and explain the difference between atom and ion size of an element.
Inversion of Configuration and Determination of R/S. Draw a compound with an asymmetric center. Rotate so that you can determine whether it is R or S. Invert the stereochemistry
Explain how long would it take to build up a lethal concentration of CO of 1000 ppmv parts per million by volume
Which of the following pairs of atomic orbitals on adjacent nuclei can overlap to form a sigma bond? Consider the x-axis as the internuclear axis
An ideal gas in a sealed container has an initial volume of 2.25 L. At constant pressure, it is cooled to 21.00C where its final volume is 1.70 L. What was the initial temperature
Calculate the net charge of Aspartic Acid. Its given that Aspartic acid has a pK1 COOH at 1.99 and also a pK2 NH3 group at 9.90
You add an excess of solid MX in 250 g water. You measure the freezing point and find it to be -0.028 degrees celsius. What is the Ksp of the solid. Assume the density of the solution is 1.0 g/cm^3.
produces carbon dioxide and water. After 5.6 of ethanol (density = 0.789 ) was allowed to burn in the presence of 12.5 of oxygen gas, 3.10 of water (density = 1.00 ) was collected. Determine the theoretical yield of H2O and the percent yield for th..
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction C2H6(g)+H2(g) 2CH4 the standard change in Gibbs free energy is
Calculate the molar mass that would be obtained from the actual experimental data under the following conditions. The unknown is methyl propyl ether (CH3OC3H7)
A reverse osmosis unit is to be used to concentrate the aqueous solution of metal complexes left over from a metal finishing operation. A pressure of 100 bar is exerted on the solution side of the membrane during concentration.
Write and ionic equation to show what happens when we add small quantities of H+ ions to a buffer solution that contains equimolar amounts
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