- Question #9f499 - Socratic
Explanation: Your starting point here is the pH of the solution More specifically, you need to use the given pH to determine the concentration of hydroxide anions, #"OH"^ (-)#, present in the saturated solution
- Question #370a7 - Socratic
The sodium ions remain in solution as spectator ions If XS sodium hydroxide is added the precipitate redissolves to give the soluble plumbate (II) ion A simple way of writing this is: (chemguideUK) Ammonia solution can't do this as the concentration of OH^ (-) ions is not high enough
- Question #c548d - Socratic
Question 1: K_ (sp)= 1 1 xx10^ (-11) Question 2: s= 4 9 xx10^ (-12)M Quest (1) determine the ksp for magnesium hydroxide Mg (OH)_2 where the molar solubility of Mg
- Calculating the concentration of excess HCL in E - Socratic
The acid in excess is then titrated with N aOH (aq) of KNOWN concentration we can thus get back to the concentration or molar quantity of M (OH)2 as it stands the question (and answer) are hypothetical
- Question #e7848 - Socratic
Similarly, OH^- becomes H_2O, indicating a gain of a H^+ ion So, you can say that NH_4^+ is the acid, and OH^- is the base Conjugates are basically the "other" term For every acid, you have a conjugate base (that no longer has that extra H^+ ion), and for every base, you have a conjugate acid (that has an extra H^+ ion)
- Question #d6b18 - Socratic
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 : Ca +H_2+O_2->Ca (OH)_2 Let us now write down the given equations: [The first equation mentioned is incorrect, and so I have revised it ] (1) 2H_2 (g) + O_2 (g)->2H_2O (l) and DeltaH_1=-571 66 kJmol^-1 (2) CaO (s) + H_2O (l
- Question #750c8 - Socratic
Here's what I got The problem wants you to use the base dissociation constant, K_b, of ammonia, "NH"_3, to determine the percent of ammonia molecules that ionize to produce ammonium cations, "NH"_4^(+), and hydroxide anions, "OH"^(-) As you know, ammonia is a weak base, which means that it does not ionize completely in aqueous solution Simply put, some molecules of ammonia will accept a
- Question #32390 + Example - Socratic
Ca(OH)2 (s] ⇌ Ca2+ (aq] + 2OH− (aq] Since calcium hydroxide is formed when two hydroxide anions bond ionically with one calcium cation, dissolving one mole of the solid in aqueous solution will of course produce one mole of calcium cations and two moles of hydroxide anions
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