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What else can I help you with?
Exceptions of Cl-, Br-, I-?
Ag, Hg, Pb
What interpretation can be made from AgBr gives Ag plus Br?
dissociation reaction
How do you set up the equation to determine the concentrations of silver ions and bromide ions given the balanced equation AgBr Ag Br- the Ksp value of silver bromide at 25 degrees is 5x10-13?
[Note: The answer has been corrected as follows:] The equilibrium reaction is: AgBr(solid) <<---> Ag+aq + Br-aq A solution equilibrium constant, Ksp, is the product of the ion concentrations in water (aq): Ksp = [Ag+aq][Br-aq] = 5x10-13 and since [Ag+aq] = [Br-aq] when only AgBr is dissolved (pure solution), you can calculate (by taking square root of Ksp) that: [Ag+aq] = [Br-aq] = SQRT(5x10-13) = 7.1*10-7 mol/L By having such a small solution constant, you can hopefully see that there will be MUCH more AgBr(solid) than ions(aq), because silver bromide is rather insoluble.
What is the chemical equation for Br?
Br- is chemical symbol for a bromide anion. It is not an 'equation', it can be a part of a chemical equation, like in this precipitation reaction (example) Ag+(aq) + Br-(aq) --> AgBr(s) .
Chemical symbol for silver bromide?
the answer is Ag Br
How do you write out nuclear symbol for Ag?
Ag is the nuclear symbol for silver.
Is AgBr a element or a compound?
AgBr is a compound composed of silver (Ag) and bromine (Br) elements.
If AgNO3 solution is added to a solution containing Br ions until the silver ion concentration is 1.3x10-6 what is the Br ion concentration The ksp for AgBr is 5.2x10-23?
The ksp is defined as the product of the concentrations of the ions formed by dissolution of the solid (divided by the activity of the solid, which is conventionally taken to be 1). Therefore, [Br-] = 5.2 X 10-23/1.3 X 10-6 = 4.0 X 10-17, to the justified number of significant digits.
Calculate the molar solubility of AgBr in a 3.0 x 10-2 M silver nitrate AgNO3 solution?
AgBr + Ag(NO)3 ----------> Ag+ + Br- Disregard Ag(NO)3 b/c of the common ion Ag and the fact that (NO)3 is a spectator ion. You use the Ksp of AgBr from the index in your book that equals 5.0*10^-13 If you look at your above equation, Ksp = [Ag] [Br] You know Ksp = 5.0*10^-13 You have also been given the concentration of Ag from Ag(NO)3 = 3.0*10^-2. You use this number because remember NO3 is always a spectator ion so [Ag] will equal the [Ag(NO)3] You equation should look like this. (Forget about doing the I.C.E on this one. Its not necessary. 5.0*10^-13-= [3.0*10^-2] [Br] Simply solve for [Br] by dividing 5.0*10^-13 by 3.0*10^-2. [Br] = 1.66*10^-11. Round for sig figs to = 1.7*10-11
Most Cl, Br, and I salts are soluable notable exceptions are salts of Ag, Pb, and Hg.?
Rule 3
How did Ag engineering begin?
The write way
Are there any liquid metals beside Ag and Br?
Yes, there are other liquid metals besides silver (Ag) and bromine (Br). Some examples include mercury (Hg), gallium (Ga), and cesium (Cs). These metals have low melting points, allowing them to exist in liquid form at or near room temperature.
