A) Calculate the concentration in ppm and the molarity of Cd in a 2.00 mL sample...

A) Calculate the concentration in ppm and the molarity of Cd in a 2.00 mL sample which has been shown to contain 16.4 μg Cd. Assume the sample has a density of 1.00 g/mL.

Expert Solution

Dear student,

Please give a positive ratings to this answer.

And stay safe...

With regards...

queen_honey_blossom answered 2 years ago

Calculate the concentration in ppm and the molarity of Cd in a 2.00 mL sample which...

Calculate the concentration in ppm and the molarity of Cd in a 2.00 mL sample which has been shown to contain 16.4 μg Cd. Assume the sample has a density of 1.00 g/mL.

A 236.4 mL sample of water contains 0.0294 g of NaCl. Calculate the concentration in ppm....

A 236.4 mL sample of water contains 0.0294 g of NaCl. Calculate the concentration in ppm. concentration = ___ ppm

Calculate the final concentration (in Molarity) when 25 mL of water is added to 95 mL...

Calculate the final concentration (in Molarity) when 25 mL of water is added to 95 mL of 1.7 M LiCl. Show your work. Part E - How many grams of KCl must be added to depress the freezing point of 1.00 kg of water to a temperature of -2.0 C? Show your work. Part F - What is the maximum number of grams of KI that can be added to 40. g of water before any precipitation is formed at...

The concentration of an undiluted sample is 26.4 mg/ml. To calculate that answer, the concentration of...

The concentration of an undiluted sample is 26.4 mg/ml. To calculate that answer, the concentration of the diluted sample was multiplied by the dilution factor. Knowing that the dilution factor is 2, work backwards to determine the concentration of the DILUTED sample. A. 13.2 mg/ml B. 132.0 mg/ml C. 1.32 mg/ml D. 26.4 mg/ml What is the unit used to describe cell solutions measured in a spectrophotometer? Cells/milliliter Grams (g) Optical density (OD) Meters (m) Spectroscopy is based on the...

70.0 mL base with 2.00 M molarity is added to 80.0 mL Oxalic acid with 1.80...

70.0 mL base with 2.00 M molarity is added to 80.0 mL Oxalic acid with 1.80 M molarity. The initial temperature is 20.0 °C and specific heat capacity is assumed to be the same as water (4.184 J/ g °C). Once the reaction reached thermal equilibrium, the temperature became 32.72°C. Find the enthalpy of neutralization for base.

Also use 0.1 M NaOH. 1. The concentration (molarity) of H3PO4 in your 250.00 mL sample...

Also use 0.1 M NaOH. 1. The concentration (molarity) of H3PO4 in your 250.00 mL sample using the data from part B. 2. The mass (in mg) of NaH2PO4 in the 250.00 mL sample using the data in part B. In my data: the first equivalence point is rech at 18 ml at pH 4.75, second equivalence point is reach at 47.0 mL at pH 9.85. I stop titrating at 52 mL with pH 11.00. Help Please.

Start with a 1040.0 ppm Stock Zn solution. Prepare control 1 by diluting 2.00 mL of...

Start with a 1040.0 ppm Stock Zn solution. Prepare control 1 by diluting 2.00 mL of Stock Zn solution in a 200.0 mL volumetric flask and dilute to the mark. Prepare control 2 by diluting 2.00 mL of control 1 into a 100.0 mL volumetric flask. What is the Zn concentration (ppm Zn) in control 2?

. Give the concentration of the following in terms of Molarity. a. The molarity of...

. Give the concentration of the following in terms of Molarity. a. The molarity of hydroxide ions in a 4.25M solution of barium hydroxide. b. The molarity of sodium ions in a 11.5M sodium phosphate solution.

Calculate the molarity of an HCl solution if a volume of 39.54 mL of this solution...

Calculate the molarity of an HCl solution if a volume of 39.54 mL of this solution is required to titrate 0.2348 g Na2CO3. (Bromocresol green is used as an indicator). This HCl solution (calculated in question 1.) is then used to analyze an unknown sample. Calculate the % Na2CO3 in the sample if a volume of 23.44 mL of the HCl solution is required to titrate 0.4089 g of the sample

A sample of water with a Fe2+ concentration of 500 ppm. Additionally Eh is 0.503 V...

A sample of water with a Fe2+ concentration of 500 ppm. Additionally Eh is 0.503 V and pH is 3.45. Will Fe(OH)3(s) stay in solution? What would be the equilibrium Eh at this pH?

Question