Kearstyn

When 50.0mL of 0.100M NH3 (Kb=1.8x10^-5) solution is mixed with 20.0mL of of 0.250M HCl solution, what is the pH after reaction? I solved the ka=5.56x10^-10 and I solved the moles of each nHCl and nNH3 and both have 0.005 moles. What do I do after this? T...

I can't solve this! I keep trying but I can't get it. Suppose 25mL of 1.00M HCl is added to 50mL of 1.00M HF. What is the pH of the HF in this solution? The pH is supposed to be 0.48 Thanks. -K.

How is this question solved?! When 21.6g of a metal X are burned in excess oxygen, 40.8g of X2O3 are formed. From this data, what is the metal X?

How is this question done? The percent abundance of deuterium (2H isotope) in naturally occurring hydrogen is 1.4x10¯2 mole %. What mass, in g, of deuterium would be present in one mole of C6H12O6?

I am still completely stuck. I did this and I got 102 for the molar mass. The answer should be around 26-27; the answer posted indicates that Al is the element in question. Thanks, again.

4X + 3O2 --> 2X2O3 21.6g 40.8g Oxygen used= 40.8g-21.6g= 19.2g moles O2= 19.2 /MM = 19.2/32 = 0.6 3/0.6 = 2/x therefore, x = 0.4 moles MM=40.8/0.4 = 102 Not sure what is wrong?! Thanks very much!

Ah! That makes sense! Thanks so much!