determine the molar concentration of hydronium ions in a solution of HNO3 that has a pH of 10.
Calculate the number of grams of NaCl2, must be dissolved in 2.5o L of water to make 0.1 M solution?
what is the pH of a 0.00000001 M solution of the strong acid HBr dissolved in water?
Calculate the molar concentration of hydronium ions in a 0.00001 M solution of the strong acid HI.
Calculate the molar concentration of hydronium ions in a 0.00001 M solution of NaOH dissolved in water?
Calculate the molar concentration of hydroxide ions in solution with a pH=2.
Can anyone please help with these, i have been working on these for 5 days and cant figure them out. need answers asap. Please and Thank you. :)
Calculate the number of grams of NaCl2, must be dissolved in 2.5o L of water to make 0.1 M solution?
what is the pH of a 0.00000001 M solution of the strong acid HBr dissolved in water?
Calculate the molar concentration of hydronium ions in a 0.00001 M solution of the strong acid HI.
Calculate the molar concentration of hydronium ions in a 0.00001 M solution of NaOH dissolved in water?
Calculate the molar concentration of hydroxide ions in solution with a pH=2.
Can anyone please help with these, i have been working on these for 5 days and cant figure them out. need answers asap. Please and Thank you. :)
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One part per million is the same as one milligram per liter of water.
It looks like you have one million grams of water, and at l000 grams of water per liter you have
one million over l000g/liter = l000 liters of water.
this means that if your concentration is to be 7 parts per million, you will need 7 milligrams of NaCl for each liter of water, and it totals out 7 mg/liter times l000 liters = 7000 mg or 7 grams
with a pH of l0 you actually have a basic solution and with a pH of l0 the H+ concentration is
l x l0 - l0th moles per liter. recall (H+) = antilog (-pH)
So if the pH is l0, this means that the pOH is 4. Recall pH + pOH adds to l4.
Therefore, the moles per liter OH = l x l0-4. or you could say (OH-) = antilog (-pOH)
3. .l molar = .l mole of NaCl per liter, and if you have 2.5 liters you will need 2.5 times .l mole/liter to = .25 moles of NaCl total
Add up the atomic wts in NaCl, 23 + 35.5 to get 58.5 grams per mole.
you need .25 moles, so multiply .25 times 58.5 grams per mole to get 14.6 grams NaCl needed
4. The molarity of the HBr = l x l0-8 moles per liter and it is a strong acid so the (H+) concentration must also be l x l0-8 moles per liter because strong acids in dilute solutions ionize close to l00%
It looks like you have one million grams of water, and at l000 grams of water per liter you have
one million over l000g/liter = l000 liters of water.
this means that if your concentration is to be 7 parts per million, you will need 7 milligrams of NaCl for each liter of water, and it totals out 7 mg/liter times l000 liters = 7000 mg or 7 grams
with a pH of l0 you actually have a basic solution and with a pH of l0 the H+ concentration is
l x l0 - l0th moles per liter. recall (H+) = antilog (-pH)
So if the pH is l0, this means that the pOH is 4. Recall pH + pOH adds to l4.
Therefore, the moles per liter OH = l x l0-4. or you could say (OH-) = antilog (-pOH)
3. .l molar = .l mole of NaCl per liter, and if you have 2.5 liters you will need 2.5 times .l mole/liter to = .25 moles of NaCl total
Add up the atomic wts in NaCl, 23 + 35.5 to get 58.5 grams per mole.
you need .25 moles, so multiply .25 times 58.5 grams per mole to get 14.6 grams NaCl needed
4. The molarity of the HBr = l x l0-8 moles per liter and it is a strong acid so the (H+) concentration must also be l x l0-8 moles per liter because strong acids in dilute solutions ionize close to l00%
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