Sodium borohydride and lithium aluminum hydride are two of the most commonly used reducing agents. Match the comments below to the reducing agent by dragging the statements into the appropriate box. If both reducing agents match the statement then drag the statement into the box lableled "True for both hydrides. True for onl True for only lithium aluminum hydride sodium borohydride True for both hydrides Reduces aldehydes to s the least reactive s the safest to use primary alcohols of the two hydrides. Reduces carboxylic acids Reduces esters. Can be used in reactions to primary alcohols with methanol solvent Reduces ketones to secondary alcohols

Organisms are more likely to be more preserved in mud than sand because mud is moist and wet, while sand is very dry.

It’s the energy source of stars

Answerthis solution will not form a precipitateexplanationsolubility equilbrium:         pbf₂(s)  ⇄ pb²⁺(aq) + 2 f⁻(aq)the solubility product expression is    (we exclude solids from the equilibrium expression).now suppose we have the trial ion product q, which we can define as    then, we can interpret  q as the product of the concentration of the ions that we have and ksp as the product of the ion concentrations that are needed to form a saturated solution.if q > ksp, then that implies that there will be a surplus of ions that exceed the amount that is required to form a saturated solution. a precipitate will then form (the precipitate continually  forms until the surplus ions are removed and q is decreased to ksp's value).if q = ksp, the saturated solution that forms is barely saturated and the precipitate will be minimal.if q < ksp, then the ion concentration will not be enough to form a saturated solution (so no precipitate).using our information, we calculate the trial ion product:     since q = 2.7  × 10⁻⁸ < ksp =  4  ×  10⁻⁸, a precipitate will not form.