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Calculate the pH of an KOH solution if 56.4 mL of KOH soultion is titrated with a 0.875 M HCl and it took 15.6 mL of the HCl to reach the equivalence point.
The Ka for HF is 3.5 × 10-4. What would you expect the percent ionization to be for the same concentration of hydrochloric acid (HCl)? Explain.
Which one of the following reactions occurring at 25 ?°C is the formation reaction of H2SO4(l) a. H2(g) + S(s) + 2O2(g) => H2SO4(l) b. H2SO4(l) => H2(g) + S(s) + 2O2(g) c. H2(g) + S(g) + 2O2(g) => H2SO4(l) d. H2SO4(l) => 2H(g) + S(s) + 4O(g) e. 2H..
A 0.5220 g sample of an unknown monoprotic acid was titrated with 9.98×10?2 M NaOH . The equivalence point of the titration occurs at 23.70 mL. Determine the molar mass of the unknown acid.
The vapor pressure of water at 40.0 degrees celcius is 55.32 mmHg. Calculate the vapor pressure of a solution of 1.50m K2CO3 at this temperature (assume 100% dissociation)
Calculate the molality of C2H5OH in a water solution that is prepared by mixing 50.0 mL of C2H5OH with 108.4 mL of H2O at 20°C. The density of the C2H5OH is 0.789 g/mL at 20°C. (Assume the density of water at this temperature is 1.00 g/mL.)
For HCB, log Kow = 6.6. What would be the predicted concentration (ppm) of HCB due to bio-concentration in the fat of fish that swim in waters containing 0.000010 ppm of the chemical?
The molecular weight of X is 65.0 g/mol. The heat required to melt one mole of the solid phase is 20.0 kJ, the heat required to sublime one mole of the solid phase is 40.0 kJ, and the heat required to vaporize one mole of the liquid phase is 30.0 ..
When 1.269 g of this compound (molar mass = 103.67 g/mol) was burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 6.029 °C. What is the heat capacity (calorimeter constant) of the calorimeter
Calculate the solubility of Ni(OH)2 in a) distilled water and b) at pH of 4.0. Justify your answer. I know I need to use a mass balance ans the reaction for disolution is
A gas expands and does P-V work on the surroundings equal to 337 J. At the same time, it absorbs 177 J of heat from the surroundings. Calculate the change in energy of the gas.
the specific heat of an unknown metal is found to be 0.233 j kg. The law of dulong and petit predicts a molar heat capacity of J/K mol. Use this law to estimate the molar mass of the element.
A 3.0 L bulb containing He at 129 mmHg is connected by a valve to a 2.0L bulb containing Ar at 110 mmHg. Calculate the partial pressure of each gas and total pressure after the valve between the flask is opened.
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