< since the molarity of either acid is the same, the moles of each acid are equal That means the difference between their ph is determined solely on which acid dissociates more Since the strong acid dissociates more (releases more #h^+# ions), it will have a lower ph = since both acids are monoprotic (they only release one hydrogen) they will both take the same amount of #oh. When an acid and a base are placed together, they react to neutralize the acid and base properties, producing a salt (neutralisation) The compound formed by the cation of the base and the anion of the acid is called a salt
Example h cl + n aoh → n acl + h 2o hydrochloric acid + sodium hydroxide →. The nitrate and the natrium ions Na_2co_3(aq) + 2agno_3(aq) rarr ag_2co_3(s)darr + 2nano_3(aq) the net ionic equation is This is also a 1:1 ratio. We want the standard enthalpy of formation for ca (oh)_2 Thus, our required equation is the equation where all the constituent elements combine to form the compound, i.e.
Why isn't a mixture of a strong acid and its conjugate base considered a buffered solution? M g(oh)2(s) ⇌ m g2+ (aq) + 2oh − (aq) in order to determine the maximum concentration of m g2+ ions permissible in the n aoh solution before a precipitate will be formed, you'd need the value of the solubility product constant, ksp. Because n aoh → n a+ + oh − and n i2+ + 2oh −→n i(oh)2 total mols of n aoh 60ml ⋅ 0.45m ol/l = 27mm ol of n aoh (dont forget the m for milli=one thousandth) this will produce 27 2 = 13.5mm ol of n i(oh)2 now you multiply this by the molecular mass number to get the weight in milligrams (divide by 1000 to get the grams) Nickel (ii)hydroxide may be formed without or (more likely.
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