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Compare the experimental mole ratio of NaHCO3 to NaCl with the theoretical mole ratio. Explain the difference. The experimental mole ratio is 1:1.
Aluminum reacts with excess hydrochloric acid to form aqueous aluminum chloride and 36.8 mL of hydrogen gas over water at 27°C and 764 mmHg. How many grams of aluminum reacted?
The equilibrium constant KC for the reaction 2H2(g) + CO(g) ? CH3OH(g) is 135 at a certain temperature. If there are 5.23 ? 10?2 moles of H2 and 3.73 ? 10?
The concentration of an enzyme within a cell is extremely low relative to other material present, yet functions effectively in its metabolic role.
Write the neutralization reaction, balance it, name the products THEN Solve the problem above.
An ice cube of mass 10.0g. Is at -20oC. How much energy is needed to make the ice into steam at 172oC?
Explain how you arrived at this conclusions. Write a balance chemical equation for the reaction that occurs when sodium cyanide dissolves in water.
What mass of I2 is needed to add to a 250 mL volumetric flask to produce a solution that is 0.20 M? (Enter unit as g.)
Calculate the distance (in Angstroms) and energy (KJ/mol) where the molecules are most attractive.
If 17.0 mL of 0.800 M HCl solution are needed to neutralize 5.00 mL of a household ammonia solution, what is the molar concentration of the ammonia?
an acetic acid solution of 2.87 pH is titrated with 1.5 mL of bromocresol green. When the color changes to light green, the pH is 3.95. The final color of the solution is dark blue.
A buffer is made by combining 3.50 L of 0.200M butylamine, C4H9NH2 with 7.50L of 0.100M butylammonium chloride, C4H9NH3Cl. Assuming that volumes are additive
78 mL of 2.5 M phosphoric acid is neutralized with 500 mL of potassium hydroxide. What is the concentration of the base?
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