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A titration was performed with 100 mL of 0.25 M acetic acid and 0.25 M sodium hydroxide.
a) Write the chemical equation for the neutralization reaction and identify the ACID, BASE and the SALT
b) Calculate the pH when 0 mL of base has been added (hint: no reaction has occurred yet)
c) Determine the pH when 50 mL of base has been added
d) Determine the pH when 100 mL of base has been added
pure potassiom hydrogen phthalate is used for standardization of the sodium hydroxide solution. suppose that the
dry-cleaning solvent (molecular weight = 146.99 g/mol) that contains C, H, and Cl is suspected to be a cancer-causing agent. When a 0.133 g sample was studied by combustion analysis, 0.239 g of CO2 and 0.0323 g of H2O formed. How many moles of eac..
At 57.8 °C, the vapor pressure of CCl4 is 54.0 kPa, and its enthalpy of vaporization is 33.05 kJ/mol.
Calculate the amount of heat liberated (in kJ) from 417 g of mercury when it cools from 64.0°C to 12.0°C.
The vapor pressure and enthalpy of vaporization of an unknown substance are measured to be 204.2 torr and 28.8 kJ/mol, respectively at room temperature (298.15 K). Estimate the normal boiling point of the substance at an atmospheric pressure of 76..
Suppose that a student doing this experiment used KHP that was not dry to standardize the NaOH solution. Would her calculated molarity of the NaOH solution be too high or too low
a chemistry student dissolved 500 grams of alcl3 in 2750grams of h20. the resulting solution had a density of1.015 gml.
At a certain temperature, the solubility of potassium iodate, KIO3, is 41.1 g/L. Calculate its solubility product constant for this temperature.
Express the concentration of a 0.0170 M aqueous solution of F-, in mass percentage and in parts per million. assume the density of the solution is 1.00g/ml
After the reaction, the mass of the beaker, water, and the remains of the tablet weighs 87.42 g. What was the mass of the liberated carbon dioxide gas
List at least three potentially hazardous features associated with concentrated sulfuric acid.
One of the buffers to maintain the pH of blood uses phosphoric acid, H3PO4, buffer. Phosphoric acid is triprotic and it's equilibrium constants are Ka1=7.5x10-3, Ka2=6.2x10-8, and Ka3=3.6x10-13. How would we prepare 2.0L of a phosphoric acid buffe..
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