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The pH at the ¼ neutralized point in the titration of a weak acid is 3.958. What is the pKa of this acid?
Given the following percent composition, what is the molecular formula? 40%C, 6.7% H, 53.3% O
certain substance has a temperature of 30 oC, a mass of 10.2 g and a density of 1.02 g/cm3. What will the % concentration, temperature, mass and density of 20.0 mL of this solution be?
What is the triple point of material X. Consider melting 3.00 moles of material X at 1.00 atm. Assuming that the melting co-existence curve is a straight line, what is X's normal melting temperature
Calculate the empirical formula and the molar formula.
What is the H+ concentration of an aqueous solution with a pOH= 4.38 at 25 degrees celcius.
Give the general Henderson-Hasselbalch equation and sketch the plot it describes (pH against amount of NaOH added to a weak acid). On your curve label the pKa for the weak acid, and indicate the region in which the buffering capacity of the system..
A steel tank with a volume of 9.583 L contains N2 gas under a pressure of 4.972 atm at 31.8 °C. Calculate the number of moles of N2 in the tank.
Given total pressure and equilibrium constant, calculate equilibrium partial pressure, The heterogeneous equilibrium process
At -11.0 °C (a common temperature for household freezers), what is the maximum mass of sorbitol (C6H14O6) you can add to 2.50 kg of pure water and still have the solution freeze? Assume that sorbitol is a molecular solid and does not ionize when i..
a tank with a volume of 1.00M3 is filled with air at 0 degrees to 20 times its atmospheric pressure. How much volume will occupy at 1 atom and room temp?
16.2g iron(III) chloride reacts with 3.33g NH2OH in acid to produced N2O gas. a) Write a balanced, net ionic equation.
An equilibrium mixture of this reaction(NH4HS(s)?NH3(g)+H2S(g)) at a certain temperature was found to have [H2S]= 0.350M and [NH3]= 0.276M .What is the value of the equilibrium constant (Kc) at this temperature.
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