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Calculate the concentration of the third standard solution using the dilution scheme outlined in the experiment. The initial dye solution is 1.24 mg/mL
The ionization constant or dissolution constant (KA) for acetic acid (HAc) is 1.8×10-5. (1) Write down the dissociation reaction. (2) Estimate pH of a solution containing 0.6 g of acetic acid in 1 L of water. Molecular weight of acetic acid is 60 ..
The half-cell is a chamber in the voltaic cell where one half-cell is the site of an oxidation reaction and the other half-cell is the site of a reduction reaction.
Given a buret filled with 0.12 M acetic acid and a second buret filled with 0.18 M sodium acetate, how many milliliters of each solution should be mixed together to produce 20.5 mL of a solution with a pH of 4.90?
Unit cell problem of copper (Cu) is a face-centered cube that has an edge lenth of 3.62 A (note: 1A=1*10^-10 m). Determine the volume occupied by one mole of copper atoms, , in terms of mL/mol.
What is the pH when 5.00 mL of base has been added. What volume is required to get to the first midpoint
Solid soduim reacts violently with water producing heat hydrogen and sodium hydroxide. How many moeclues of hydrogen gas are formed when 48.7 g of sodium are added to water.
As a reaction progresses backwards toward equilibrium K is the highest value Q attains. e) A reaction with no products present has an infinite Q value.
The osmotic pressure of this solution was 0.00178 atm at 25 C. Calculate the molar mass of hemoglobin, which is a molecular compound and a nonelectrolyte
Problem- If a solution containing 46.876 g of mercury(II) chlorate is allowed to react completely with a solution containing 14.334 g of sodium sulfate, how many grams of solid precipitate will be formed
The following chemical equilibria are studied in this experiment. To become familiar with their behavior, indicate the direction, left or right, of the equilibrium shift when the accompanying stress is applied to the system
PH for the reaction 2 H2O (l) H3O+(aq) + OH-(aq) is +55.8 KJ/mol. and the equilibrium constant for the reaction is Keq= 1.0x10-14. What is ?S for this reaction
Calculate the concentrations of the protonated and unprotonated forms of bromothymol blue in 100 mL of a pH 8.1 buffer solution to which 1.0 mL of a 0.005 M solution of bromothymol blue
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