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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_4oh molar mass of nh_4oh is 35.04 g/mol mass of solute = 0.18 cancelmol × 35.04 g/cancelmol = 6.3072 g < 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. 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. 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. Copper forms an insoluble hydroxide that is fairly poorly characterized Another way we could look it as a hydrated copper oxide, i.e Cuo ⋅ oh 2 ≡ cu(oh)2. Could a buffered solution be made by mixing aqueous solutions of hcl and naoh 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.