Mass spectrometry is more often applied to molecules than to atoms. we will see in chapter 3 in the textbook that the molecular weight of a molecule is the sum of the atomic weights of the atoms in the molecule. the mass spectrum of h_2 is taken under conditions that prevent decomposition into h atoms. the two naturally occurring isotopes of hydrogen are^1h (atomic mass = 1.00783 a mu; abundance 99.9885%) and^2h (atomic mass = 2.01410 a mu; abundance 0.0115%). how many peaks will the mass spectrum have? express your answer as an integer. give the relative atomic masses of each of these peaks. express your answers using six significant figures. enter your answers in ascending order separated by commas.

Relationships are difficult because people choose to walk away instead of having to try harder.

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.