The thing to keep in mind here is that nitric acid is a strong acid, which means that it will ionize completely in aqueous solution to produce hydronium cations, H3O+, and nitrate anions, NO− …

"6.3072 g" >>"Molarity" = "Moles of solute"/"Volume of solution (in litres)" "0.45 M" = "n"/"0.4 L" "n = 0.45 M × 0.4 L = 0.18 mol" You need "0.18 mol" of "NH"_4"OH" Molar mass of "NH"_4"OH" …

The balanced chemical equation for the partial dissociation of the base looks like this "BOH"_text ( (aq]) rightleftharpoons "B"_text ( (aq])^ (+) + "OH"_text ( (aq])^ (-) By definition, K_b will be …

The degree of dissociation sf (alpha=0.0158) sf (K_b=2.51xx10^ (-6)color (white) (x)"mol/l") Triethyamine is a weak base and ionises: sf ( (CH_3)_3N+H_2Orightleftharpoons …

H^+ + OH^--> H_2O when the acid was added to the resulting solution. The H^+ and OH^- react in a 1:1 ratio. This tells us that the number of moles of H^+ used will be equal to the number of …

The added water to reach "100.00 mL" doesn't change the mols of HCl present, but it does decrease the concentration by a factor of 100//40 = 2.5. Regardless, what matters for …

sf(pH=7.04) This is a very dilute solution of NaOH so I would expect the pH to be 7 or very slightly above. Because the concentration is so low we must also take into account the ions that are …

Since water is in excess, "67.7 g MgO" are needed to produce "98.0 g Mg(OH)"_2. Balanced equation "MgO(s) + H"_2"O(l)"rarr"Mg(OH)"_2("s")" Moles magnesium hydroxide Start with the …

pH = 1.61151 OH^- = 4.08797 * 10 ^-13M HF = 0.855538M H^+ = 0.024462M F^- = 0.024462M HF + H_2O = H_3O^+ + F^- We can find the concentration of H^+ or H_3O^+ by three ways …

Here's what I got. Start by writing the balanced chemical equation for this neutralization reaction. Since sodium hydroxide is a strong base that dissociates completely in aqueous solution, you …