substance that have the right to either shed or accept a proton (H+ion): can role as either Bronsted-Lowry acid or basic (H20)
-Bronsted-Lowry acid donates a proton (H+).

You are watching: Write a net ionic equation to show that nitric acid, hno3, behaves as an acid in water.

-HCN donates a proton come H2O to type CN- .HCN (aq) + H2O CN- (aq) + H3O+ (aq)
Write a network ionic equation to display that caffeine, C8H10N4O2, behaves together a Bronsted-Lowry base in water.
-Bronsted-Lowry base accepts a proton (H+).-C8H10N4O2 accepts a proton from H2O to kind HC8H10N4O2+ .C8H10N4O2 (aq) + H2O--> HC8H10N4O2+ (aq) + OH- (aq)
.1. Include H+ to type the conjugate acid. + =2. Eliminate H+ to form the conjugate basic . = + Note: is AMPHIPROTIC: act as a Brønsted-Lowry acid/base.
When no other substances are dissolved in water, what have to be true around the concentrations of and also created by this reaction?
The hydroxide ion concentration in one (aq)solution at 25°C is 8.9×10-2 M.The hydronium ion concentration is M...The pH that this systems is...The pOH is...
In this systems = 8.9×10-2 M= (Kw/) =(Kw/8.9×10^-2M) = 1.1×10^-13 M pH =-log =-log(1.1×10-13) = 12.95=pHpOH= 14.00 - pH = 14.00 - 12.95 = 1.05=pOH
The pH of an aqueous solution at 25°C was found to it is in 13.00.The pOH of this solution is...The hydronium ion concentration is M...The hydroxide ion concentration is M....
In this solution pH = 13.00pOH = 14.00 - 13.00 = 1.00=pOH =10^-pH =10^-13.00 =1.0×10^-13 M= 10^- pOH = 10^- 1.00 = 0.10 M
What is the pH that a 3.55×10-4 M systems of the strong acid HCl?HCl(aq) + H2O(ℓ) → Cl-(aq) + H3O+(aq)0 = 3.55×10-4
Determine Hydronium Ion Concentration-Ionization that a solid acid top top dissolution in H2O is suspect to it is in 100% complete.HCl(aq) + H2O(ℓ) → Cl-(aq) + H3O+(aq)-So, =subscript0 = 3.55×10-4Determine pH-pH=-log =-log(3.55×10-4) = 3.45
Determine -=strong base: 100% ionized in H2O: 1mol KOH outcomes in 1mol the in solution. -So, = 4.7×10-2 mol/L. Kw = = 1.0 × 10^-14 =Kw/ =1x10^-14/4.7x10^-2 =2.1x10-13 mol/LDetermine pH pH= -log = -log(2.1×10-13) = 12.67
HCl: Hydrochloric acidHNO3: Nitric acidH2SO4: Sulfuric acidHBr: Hydrobromic acidHI: Hydroiodic acid (also known as hydriodic acid)HClO4: Perchloric acidHClO3: Chloric acid
LiOH - lithium hydroxideNaOH - salt hydroxideKOH - potassium hydroxideRbOH - rubidium hydroxideCsOH - cesium hydroxide*Ca(OH)2 - calcium hydroxide*Sr(OH)2 - strontium hydroxide*Ba(OH)2 - barium hydroxide* these bases completely dissociate in remedies of 0.01 M or less. The other bases make solutions of 1.0 M and also are 100% dissociated at the concentration. There room other strong bases than those listed, yet they space not often encountered.

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What is the hydronium ion concentration in one aqueous nitric acid solution that has a pOH that 11.920? = M??
Since nitric mountain is a solid acid, the dissociates basically 100%. + --> + I x 0M 0MC -x +x +xE 0M x xpOH = 11.920pH = 14 - pOH = -log = 14-11.920 = 2.080x = = 10 ^- pH = 10 ^- 2.080 = 8.32×10-3 M
What concentration the barium hydroxide is necessary to give an aqueous solution with a pOH the 2.080?Molarity that barium hydroxide = M??
Since barium hydroxide is a strong base, it ionizes basically 100%. Ba(OH)2--> + 2-I x 0M 0MC -x + x +2xE 0M x 2xpOH = 2.080= 2x = 10^-pOH = 10^-2.080 = 8.32×10-3 M= x = / 2 =8.32×10-3 M/ 2 = 4.16×10-3 M
Write the Ka expression because that an aqueous solution of acetic acid:(Note that either the numerator or denominator may contain more than one chemistry species. Get in the complete numerator in the optimal box and also the finish denominator in the bottom box. Psychic to write the hydronium ion out as not H+)
The weak mountain equilibrium the occurs in an aqueous equipment of acetic acid is:Ka =/H2O no in eq constant expression

The value of Ka for hydrocyanic acid , HCN , is 4.00×10-10 .Write the equation because that the reaction that goes with this equilibrium constant. (Use H3O+ instead of H+.)
Ka is the symbol for the equilibrium consistent for the reaction in i beg your pardon a weak mountain donates a proton to water to type its conjugate base and H3O+. For hydrocyanic acid this equilibrium is:(aq) + ⇄ H3O+(aq) + CN-(aq)
The link dimethylamine, (CH3)2NH, is a weak basic when liquified in water. Compose the Kb expression because that the weak base equilibrium the occurs in an aqueous solution of dimethylamine:
The value of Kb for pyridine, C5H5N, is 1.50×10-9.Write the equation for the reaction that goes v this equilibrium constant.
Kb is the symbol for the equilibrium consistent for the reaction in i beg your pardon a weak basic accepts a proton from water to kind its conjugate acid and OH-. For pyridine this equilibrium is: + +
1. Compose the Equilibrium continuous ExpressionHA(aq) + H2O(ℓ) ⇄ H3O+(aq) + A-(aq)2.Determine Hydronium Ion Concentration =10^-pH= 10-2.63 = 2.34×10-3 mol/L3. ICE recognize All Eq Concentrations = = 2.34×10-3 mol/L = 0.1077 mol/LKa=*/    