Asaturated solution prepared at 70∘c contains 32.0 g cuso4 per 100.0 g solution. a 350 −g sample of this solution is then cooled to 0∘c and cuso4⋅5h2o crystallizes out. if the concentration of a saturated solution at 0∘c is 12.5 gcuso4/100 g soln, what mass of cuso4⋅5h2o would be obtained? [hint: note that the solution composition is stated in terms of cuso4 and that the solid that crystallizes is the hydrate cuso4⋅5h2o.] express your answer using two significant figures.

Explanation:

 gram of Copper sulphate in 350 g solution is 32 x 3.5 = 112

in term of mol = 112 / 159.5 = 0.7022

after crystallisation, gm of copper sulphate in the solution

= 43.75

in term of mole

43.75/159.5 = 0.2743

mole that got precipitated in hydrated form = 0.7022 - 0.2743 =0.4279

in terms of gm of hydrated copper sulphate = .4279 x mol weight of hydrated copper sulphate = .4279 x 249.5 = 106.76 g .

Explanation:

Hello,

In this case, the mass of copper (II) sulfate that are available for the 350-g sample is:

And the mass of water:

Now, the dissolved copper (II) sulfate at 0°C is:

Therefore, the undissolved copper (II) sulfate is:

In addition, 238 g of water are equivalent to 13.5 moles of water, nevertheless, as a pentahydrate is obtained, 5 moles of water correspond to:

Therefore, the mass of copper (II) sulfate pentahydrate turns out:

Best regards.

answer: e.   sour taste

explanation: acids are those substances which dissociates in water to give ions. as they dissociate to give ions, they act as electrolytes and thus are electrically conductive. acids are sour in taste. example: hcl

bases are those substances which dissociates in water to give ions or accepts ions. as they dissociate to give ions, they act as electrolytes and thus are electrically conductive. bases are bitter in taste. bases are slippery in nature.