Search results

please help to differentiate the following (i) logx3 (ii) logx(3^x) (iii) y = x^x (iv) y = x^(logx) (v) y = x^(1/x) thanks in advance

i always thought the HF bond was a hydrogen bond which is of the strongest Van Der Waals forces. isnt it hydrogen to fluorine, oxygen and nitrogen represent hydrogen bonds. correct me if im wrong

another way is to sub z = x + iy as Mountain Dew suggests thus mod ( x + iy +1) =< mod (x +iy) + 1 i.e sqrt ( (x+1)^2 + y^2) <= sqrt (x^2 + y^2) +1 squaring both sides, we get, x^2 + 2x + 1 + y^2 <= x^2 +y^2 + 2sqrt(x^2 + y^2) +1 cancelling, we get, x<= sqrt(x^2 + y^2) squaring both sides...

Therefore Mg(OH)2 is NOT a strong base, since it is NOT soluble in water.The same person that posted this question, posted another question in a different thread enquiring as to why HF(aq) is a weak acid and HCl(aq) is a strong acid. The same theory explained here is behind this phenomena as...

thats right, thanks heaps

dont worry about the first one, i got it

please help to differentiate: (i) e^(x+logx) (ii) 3^(-1/x) i thought i could do them, but my answers are different to the back.

why didnt i see that, it so simple. thanks

HCl forms a strong acid. HF forms a weak acid. But, why should this be so if we compare the structure of these two molecules, HF is so much more polar, since fluorine is so much more elctronegative than Cl, so the HF molecule is more "egg" shaped and the H atom is a lot more loosely held (or I...

Chemistry Contexts 2, pg 160, states "all group 1 and 2 metal hydroxides are strong bases....The group 2 metal hydroxides, howver, have limited solubility. Magnesium hydroxide is vitually insoluble....To the extent to these compounds dissolve they are completely dissociated and are therefire...

Mg(OH)2 is considered a strong base, right? If so, that means it dissociates completely in solution (or almost completely). But Mg(OH)2 has a very limited solubility, so why is it referred to as a strong base? any help is appreciated - thankyou