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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 Why isn't a mixture of a strong acid and its conjugate base considered a buffered solution? 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 Could a buffered solution be made by mixing aqueous solutions of hcl and naoh Example h cl + n aoh → n acl + h 2o hydrochloric acid + sodium hydroxide →.

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. Oxidation number/oxidation state is an empirical construct, it is formally the charge left on the central metal atom when all the bonds are broken, with the charge devolving to the most electronegative atom On the pauling scale, we can quote the electronegativities of c,h, and o as 2.55,2.20,3.44 The means that the oxidation number of c in methane, ch 4, is −i v, and the oxidation number.

For oxyacids with the same number of oh groups and the same number of o atoms, acid strength increases with increasing electronegativity of the central atom Since p is more electronegative than as, we predict that h3po4 should be a stronger acid than h3aso4. 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.

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