1.If a container that is 1L has 1 mol of solid NACL , if you add more nacl will the concentration of solid increase? it should? because if you increase it to two mols it will become 2 mol/l right?
so in a equillibrium system like nacl(s)--><---na+ + cl- if you increase amount of solid the concentration would increas and so sytem would shift right?
2. if you have a container of 2(som gas)---><---(another gas) and the first gas which has two mols is brown and the gas on product side is colorless how come when pressure is increased the gas becomes darker than lighter? is it because equillibrium is distrubed and more purple gas is there than colorless gas but eventually equillibirum i sestablish again and gas becomes lighter?
3.h2so4 is diprotic what about 2hso4?
4. no matter if a solution becomes more dilute or concentratated a strogng acid and weak base dissociate 100% what if it is a weak acid and weak base does concentration or dilution affect how much it dissociates.
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5. addinf water to a equillbrium system will make it more dilute and increase the volume but decrease pressure so system will shift in direction which produces more ions?
6. dilution can also decrease rate of raction because you deacrease concentration?
First, a comment. Small letters don't do it with equations. Lower case doesn't means the same thing, sometimes, as upper case. Some of your questions I can't answer for I think what you have posted may be part of a question and I've learned not to mess with half a pig in a poke.
1.If a container that is 1L has 1 mol of solid NACL , if you add more nacl will the concentration of solid increase? it should? because if you increase it to two mols it will become 2 mol/l right?
The amount of solid will increase, of course. But by definition, the concentration of a solid (more technically, the activity of a substance in its normal state) is 1. Look at it another way. Suppose we place 1 L of water, a liquid in its normal state, in a 2 L container. What is its concentration. The concentration is 1000g/18 g/mol = 55.5 moles/L. Now let's add a L of water to the 1L that already there. What is the concentration? Now we have 2000 g and 2000/18 g/mol = 111 moles/2 L = 55.5 moles/L. Didn't change. Finally, if you are doing something with equilibrium constants, solid NaCl doesn't have a K, except, perhaps, for an equilibrium between the solid and the vapor.
The amount of solid will increase, of course. But by definition, the concentration of a solid (more technically, the activity of a substance in its normal state) is 1. Look at it another way. Suppose we place 1 L of water, a liquid in its normal state, in a 2 L container. What is its concentration. The concentration is 1000g/18 g/mol = 55.5 moles/L. Now let's add a L of water to the 1L that already there. What is the concentration? Now we have 2000 g and 2000/18 g/mol = 111 moles/2 L = 55.5 moles/L. Didn't change. Finally, if you are doing something with equilibrium constants, solid NaCl doesn't have a K, except, perhaps, for an equilibrium between the solid and the vapor.
2. if you have a container of 2(som gas)---><---(another gas) and the first gas which has two mols is brown and the gas on product side is colorless how come when pressure is increased the gas becomes darker than lighter? is it because equillibrium is distrubed and more purple gas is there than colorless gas but eventually equillibirum i sestablish again and gas becomes lighter?
I don't get it. You have a brown gas and a colorless gas. Where did the purple gas come from?
I don't get it. You have a brown gas and a colorless gas. Where did the purple gas come from?
3.h2so4 is diprotic what about 2hso4?
I assume you mean H2SO4 (and not h2so4). Yes, H2SO4 is diprotic because it has two H atoms, both which ionize. HSO4^- is monoprotic because it has only one H atom to ionize. 2HSO4^- is just two moles of a monoprotic acid, HSO4^-.
I assume you mean H2SO4 (and not h2so4). Yes, H2SO4 is diprotic because it has two H atoms, both which ionize. HSO4^- is monoprotic because it has only one H atom to ionize. 2HSO4^- is just two moles of a monoprotic acid, HSO4^-.
yeah sorry number 2 assume the purple gas ir brown
The statement is not true. A strong acid or strong base dissociate 100% in dilute or concentrated solution. However, a weak base does not dissociate 100% and it doesn't matter if it is concentrated or dilute. The second part of the question--A weak acid or a weak base dissociate to some extent, depending upon the concentration and the particular weak acid or weak base. But as water is added and the solution becomes more and more dilute, both a weak acid AND a weak base (individually) will dissociate more and more.
again a typing error sorry i meant strong acid and strong base.
On #2, yes, I think you are right. The increase in pressure immediately causes the volume of the brown gas to decrease which means the concn is higher, hence the darker color. But equilibrium will move it back and the end product is more of the gas on the right which is colorless.
so the reason why the dissociate more and more in dilute substance is because there is more h20 basically and in a more concentrated solution these is less?
You see why we recommend posting only one post or two short ones per post. It gets confusing trying to go back and answers parts of a question.
As a follow up to your weak acid/weak base and dissociation: Of course it's because there is more water but the reason why it dissociates more is because of Le Chatelier's Principal.
Take acetic acid as an example.
HC2H3O2 + H2O ==> H3O^+ + C2H3O2^-
Notice that as we add more water to the system, the reaction shifts to the right, producing more ions, and more ions mean a higher degree of dissociation. Technically, at infinite dilute (but we can't reach infinity), the solution would be 100% dissociated.
As a follow up to your weak acid/weak base and dissociation: Of course it's because there is more water but the reason why it dissociates more is because of Le Chatelier's Principal.
Take acetic acid as an example.
HC2H3O2 + H2O ==> H3O^+ + C2H3O2^-
Notice that as we add more water to the system, the reaction shifts to the right, producing more ions, and more ions mean a higher degree of dissociation. Technically, at infinite dilute (but we can't reach infinity), the solution would be 100% dissociated.
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