Chemistry Homework Solutions
#162311
An analytical chemist determines that an estuarine water sample contains 1.5 g/L of sulfate ion.
An analytical chemist determines that an estuarine water sample contains 1.5 g/L of sulfate ion. What is the concentration in terms of
(a) g/L of S
(b) molar concentration of sulfate
(c) normality
(d) parts per million of sulfate
Could you please explain what formula and step are invovled and please provide (example) problem.
What is this?
By OTA - Overall OTA Rating
Vinh (Vincent) Dang, PhD - 4.8/5
Purchase Cost Now
$2.19 CAD (was ~$7.98)
Included in Download
- Plain text response
Why you can trust BrainMass.com
- Your Information is Secure
- Best Online Academic Help Service
- Students find real academic Success
- An analytical chemist determines that an estuarine water sample contains 1.5 g/L of sulfate ion. - 5. An analytical chemist determines that an estuarine water sample contains 1.5 g/L of sulfate ion. What is the concentration in terms of (a) g/L of S (b) molar concentration of sulfate (c) normality ...
- Calculating the normality of a 1.50 M solution of H3PO4. - What is the normality of a 1.50 M solution of H3PO4?
- Convert to mg/L from Molarity - Convert to mg/L using dimensional analysis: 0.01 N Ca+2. Here is additional info: salt is CaCl2 1M HCO3 0.02 N H2SO4 0.02 M SO4 2- (i.e)sulfate ion
- ARCHAEOLOGICAL CHEMISTRY - Answer the following questions, showing calculations and equations where appropriate: 1. Your analytical technique directly and accurately measures the concentration of iron-54 in your samples. How ...
- Molarity and Normality - 50.00 mL of 0.2500M H2SO4 is titrated to a neutral endpoint with 56.03 mL of LiOH. What is the molarity and normality of the LiOH?
