A geochemist in the field takes a 36.0 mL sample of water from a rock pool lined with crystals of a certain mineral compound X.
He notes the temperature of the pool, 170 C, and caps the sample carefully. Back in the lab, the geochemist filters the sample and then evaporates all the water under vacuum. Crystals of are left behind. The researcher washes, dries and weighs the crystals. They weigh 3.96 g. Using only the information above, can you calculate the solubility of X in water at 17.0C? If you said yes, calculate it.
Yes, 0.11g/mL is the solubility of X in water at 17.0°C.
Explanation:
As the sample of water has crystals around it, the solution is oversaturated at 17.0°C. The water contains the maximum amount of X at 17.0°C, this concentration is called <em>solubility</em>. Thus, yes, we can calculate solubility in water at 17.0°C
The concentration of the crystals is 3.96g in 36.0mL, that is:
3.96g / 36.0mL =
<h3>0.11g/mL is the solubility of X in water at 17.0°C</h3>
Answer:The green growing on the penny of copper and the rust forming on the nail of iron are chemical changes. Boiling away salt water, scraping iron filings from a mixture of sand with a magnet, and breaking a rock with a hammer, are physical changes.
