# chemistry

posted by .

a 1.00 L aqueous solution contained 5.80 g of NaOH. what is the pH of the solution?
Can someone help me out with the setup of this?

• chemistry -

M = moles/L
moles = grams/molar mass
moles NaOH = 5.80 g/40 = moles and that will be the molarity since it is in 1 L of solution.
Then pOH = -log(OH^-) and pH + pOH = 14.

• chemistry -

okay, can the ph go over 14?
5.80/40=1.45
-log(1.45)= -0.16
14-^-0.16= 14.16
i must be doing something wrong

• chemistry -

No, you're doing it right. It's the problems that make it do this. The pH can be negative numbers and if these are pOH numbers, then pH will be larger than 14. In real world chemistry, it isn't the concn that is plugged into that formula but the activity of the solution. The activity approaches the concn at very very dilute solutions but at higher concns there are large deviations from so-called ideal behavior. Also, water has a leveling effect so that, in theory at least, 14 is the maximum number. Neither activity nor leveling effect get much discussion in beginning courses. I wouldn't let this bother me. Just go ahead and calculate using pH = -log(H^+) and pH pOH = 14.

• chemistry -

5.80/40 is 0.145

## Similar Questions

1. ### CHemistry

im not sure how u solve these types of problems... How many moles of NaOH are contained in 200ml of a 0.1M of NaOH?
2. ### Honors Chemistry

If 20 mL of 0.01 M aqueous HCl is required to neutralize 30 mL of an aqueous solution of NaOH, determine the molarity of the NaOH solution. ==> I got 0.01 M NaOH as my answer. Is this correct?
3. ### Chemistry

I'm trying to find the solubility of Ca(OH)2 in .0125 mol/L aqueous NaOH. Here is my data: Vol of solution used per titration: 20mL Conc of HCl: .1201 mol/L Average Titre: 4.71 I need to calculte: 1. the TOTAL [OH-] in the saturated …
4. ### chemistry

the density of a certain aqueous solution is 1.17g/ml, and the solution is 3.57% by mass NaOH. how many mL of this solution would you need to use in order to prepare 100.0 mL of .150 M NaOH solution?
5. ### CHEMISTRY

A student needed to standardize a solution of NaOH which was approximately 0.125 M. The student carefully prepared the titration setup, but after 25 mL of NaOH was added, what was the pH of solution if initially flask contains 25 mL …
6. ### chemistry

A student needed to standardize a solution of NaOH which was approximately 0.125 M. The student carefully prepared the titration setup, but after 25 mL of NaOH was added, what was the pH of solution if initially flask contains 25 mL …
7. ### Chemistry

How do I solve these problems You have 2000. g of aqueous NaOH solution. The percent by mass of the solute is 4.25%. How many grams of NaOH are in the solution?
8. ### chemistry

5.0 mL of H2SO4 solution was titrated with 0.20 M NaOH standard solution. The volume of NaOH needed to reach the equivalent point was 9.5 mL. 1. In this titration setup, what is the titrant?
9. ### Chemistry

Three bottles lost their labels. One contained an aqueous solution of HCl, another an aqueous solution of HNO3, and the third contained an aqueous solution of H2SO4. Write an experimental procedure that would allow you to correctly …
10. ### Chemistry

Three bottles lost their labels. One contained an aqueous solution of HCl, another an aqueous solution of HNO3, and the third contained an aqueous solution of H2SO4. Write an experimental procedure that would allow you to correctly …

More Similar Questions