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1. At a certain temperature, the pH of a neutral solution is 7.67. What is the value of Kw at that temperature?
2. What is the pH of a neutral solution at a temperature where Kw=8.0×10-14?
3. Calculate the pH of a solution prepared by dissolving 0.40 g of BaO in enough water to make 0.600 L of solution.
4. The temperature for each solution is carried out at approximately 297 K where Kw=1.00×10-14 0.50 g of hydrogen chloride (HCl) is dissolved in water to make 6.0 L of solution. What is the pH of the resulting hydrochloric acid solution?
Express the pH numerically to two decimal places.
0.75 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 5.5 L of solution. What is the pH of this solution?
An alkyne of six carbon atoms gives the same single product in its reaction either with BH3 in THF followed by H2O2 /OH-, or with H2O/Hg2 /H3O . Draw the structure of the alkyne (containing only carbon and hydrogen atoms).
A gas is compressed from initial volume of 5.60L to 1.23L by an external pressure of 1.00atm. During the compression the gas releases 128J of hear. What is the internal energy of the gas?
The titration is monitored with a potentiometer using a SCE reference electrode (Eref= 0.241V). the solution is buffered at ph=4.00.
Acetate ion and acetic acid in a 6-liter solution to which have been added .24 mole of HCl and 0.64 mole of sodium acetate
At the end of the process, the pressure is 2.50x10 to the 6 Pa. Calculate the final temperature of the gas. Calculate q, w, deltaU, and deltaH for this process.
Consider 4.30 L of a gas at 365mmHG and 20 C. . If the container is compressed to 2.70L and the temperature is increased to 31 C, what is the new pressure,P2 , inside the container? Assume no change in the amount of gas inside the cylinder.
2) Calculate the concentration of an aqeuous solution of Ca(OH)2 pH of 12.05.
Calculate the number of moles of H2O that will be produced by the reaction of .530 moles of solid Al(OH)3 with excess aqueous HClO3
A fixed amount of gas at 35oC occupies a volume of 10.0 L when the pressure is 876 torr. Calculate the pressure in (torr) when the volume is reduced to 7.98 L at constant temperature of 35oC
NH4NO3(s) is dissolved in water
When relatively small amounts of magnesium burns, the fires are extinguished using commercially available dry powder. Why might this fire rekindle days later as someone tries to remove the residue with water?
Given 100.0mL of a buffer that is 0.50 M in HOCl and 0.40 M in NaOCl, what is the pH after 10.0mL of 1.0 M NaOH has been added. (Ka for HOCl = 3.5 x 10^-8)
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