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NH3 is a weak base (Kb = 1.8 x 10^-5) and so the salt NH4Cl acts as a weak acid. What is the pH of a solution that is 0.044 M in NH4CL?
A solution containing 100 g of an unknown liquid and 900 g water has a freezing point of - 3.33 oC. What is the molar mass of the liquid? Kf = 1.86oC/m
What happens when the base solution was added to the acid solution but was not stirred while temperature measurements were made
Which species is the best reducing agent?
Compute the number of electrons in a flake of pure gold valued at $0.51. Assume that the price of gold
The variation of stress-concentration factor for a bar with fillet that is axially loaded shows that the kt approached infinity as the r/d ratio decrease.
When measuring horse radish peroxidase you found that a purified preparation has a specific activity of 10mmolar/sec/mg protein. suppose you added to an assay a competitive inhibitor that would not produce a colored product.
A concentrated solution of compound A in the same solvent was diluted from an initial volume of 2.00 ml to a final volume of 25.00 mL and then had an absorbance of 0.733. What is the concentration of A in the concentrated solution
A solution is made by dissolving 0.45 moles of LiCl to make 150 mL of aqueous solution. What is the molarity of the solution?
What is the osmotic pressure of a homogenous solution at the temperature At 25 o C, as this solution is consisting of 21.0 g urea
Estimate the average rate of production (Using this rate) of oxygen over the same time period. Considering the given equation 2H 2 O 2 --> 2H 2 O+O 2 -H 2 O 2
A beaker with 1.50×102mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 7.20mL of a 0.330\it M \rm HCl solution to the beaker.
A water sample is suspected to be contaminated by iron (III) ions. How could you determine if the sample is really contaminated
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