The chemical equilibrium will be unaffected
H3PO4 + H2O <--> H3O+ + H2PO4- Ka1= ([H3O+][H2PO4-])/[H3PO4])
H2PO4- + H2O <--> H3O+ + HPO4^2- Ka2= ([H3O+][HPO4^2-])/[H2PO4-])
HPO4^2- + H2O <--> H3O+ PO4^3- Ka3= ([H3O+][PO4^3-])/[HPO4^2-])
Ka1 >> Ka2 = almost all the H3O+ is formed in the first step.
Ka3 will only happen under very basic conditions.
Answer:
A=covalent B=low melting point
Explanation:
just did this on edge... not sure if it is still needed but there wasn't an answer so :)
Answer:
38.8 mL
Explanation:
2CO(g) + O₂(g)⟶2CO₂(g)
Because pressure and temperature remain constant, we can <em>think of the moles ratios as volume ratios</em>. This means that 2mL of CO react with 1 mL of O₂ to produce 2 mL of CO₂.
Because the problem asks us to calculate the amount of oxygen gas unreacted, then CO is the limiting reactant. We <u>calculate the amount of O₂ that reacted</u>, from the available amount of CO:
82.4 mL CO *
= 41.2 mL O₂
Thus, the oxygen gas remaining is:
80.0 mL - 41.2 mL = 38.8 mL O₂
It is B balance, because it has a 0,01 g divisions scale. The minimun division in A balance is only 0,1 g, i.e, decigram measurement.