Question

One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is by titrating a sample of silver nitrate solution. Any chloride anions in solution will combine with the silver cations to produce bright white silver chloride precipitate. Suppose an EPA chemist tests a 250. mL sample of groundwater known to be contaminated with nickel(II) chloride, which would react with silver nitrate solution like this: NiCl2(aq) + 2 AgNO3(aq) ? 2 AgCl(s) + Ni(NO3)2(aq) The chemist adds 80.0 mM silver nitrate solution to the sample until silver chloride stops forming. She then washes, dries, and weighs the precipitate. She finds she has collected 8.7 mg of silver chloride. Calculate the concentration of nickel(II) chloride contaminant in the original groundwater sample. Be sure your answer has the correct number of significant digits.

          One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is by titrating a sample of silver nitrate solution. Any chloride anions in solution will combine with the silver cations to produce bright white silver chloride precipitate.

Suppose an EPA chemist tests a 250. mL sample of groundwater known to be contaminated with nickel(II) chloride, which would react with silver nitrate solution like this:

NiCl2(aq) + 2 AgNO3(aq) ? 2 AgCl(s) + Ni(NO3)2(aq)

The chemist adds 80.0 mM silver nitrate solution to the sample until silver chloride stops forming. She then washes, dries, and weighs the precipitate. She finds she has collected 8.7 mg of silver chloride.

Calculate the concentration of nickel(II) chloride contaminant in the original groundwater sample. Be sure your answer has the correct number of significant digits.

Show more…

One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is by titrating a sample of silver nitrate solution. Any chloride anions in solution will combine with the silver cations to produce bright white silver chloride precipitate.

Suppose an EPA chemist tests a 250. mL sample of groundwater known to be contaminated with nickel(II) chloride, which would react with silver nitrate solution like this:

NiCl2(aq) + 2 AgNO3(aq) ? 2 AgCl(s) + Ni(NO3)2(aq)

The chemist adds 80.0 mM silver nitrate solution to the sample until silver chloride stops forming. She then washes, dries, and weighs the precipitate. She finds she has collected 8.7 mg of silver chloride.

Calculate the concentration of nickel(II) chloride contaminant in the original groundwater sample. Be sure your answer has the correct number of significant digits.

Added by Analise G.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Dominique Jan Tan

12/23/2021

Step 1

First, we need to know the volume of the original groundwater sample and the amount of nickel(II) chloride found in it. These details are not provided in the question. Show more…

Show all steps

lock

Thanks for your feedback!

Play audio

Feedback

Powered by NumerAI

Dominique Jan Tan and 56 other subject Chemistry 101 educators are ready to help you.

Ask a new question

Labs

Want to see this concept in action?

NEW

Explore this concept interactively to see how it behaves as you change inputs.

View Labs

Key Concepts

Recommended Videos

Recommended Textbooks

Transcript

00:01 Good day, the topic is about stochometry.

00:03 This is tautometry, we relate the quantities of substances in a chemical reaction.

00:08 Even the reaction between nickel -2 chloride and silver nitrate, producing agcl precipitate and nickel -2 nitrate.

00:16 It is found out that the mass of precipitate agcl formed is 8 .7 milligrams.

00:23 In the sample, that is 250 ml, we wish to find the concentration of nickel -2 chloride in really comes per m l in the original sample.

00:35 So to start, we need to first take note of the following relationship from the balance equation.

00:43 One mole of nicl2 equals two moles of agcl.

00:51 We get this from the coefficients of the balanced chemical equation.

00:57 Moreover, let us take note of the molar masses of nicl2 and agcll.

01:03 We obtained the molar mass as the sum of the atomic mass of all the atoms that make up the compound.

01:09 For example, for ag cl, we have ag, the atomic mass of ag and the atomic mass of cl in grams per mole.

01:19 That is 107 .9 plus 35 .45 respectively.

01:26 So that the atomic, the molar mass of agcl in grams per mole is equal to 143 .4.

01:37 Doing the same process, we also write the molar mass of nicl2 as 129 .6.

01:49 Now we will use dimensional analysis to solve for the milligrams of nicl 2 needed to form the given mass of agcl...

Ace is your personal tutor. It breaks down any question with clear steps so you can learn.

Start Using Ace

Continue solving this problem

Create a free account to:

View full step-by-step solution
Ask follow-up questions with Ace AI
Save progress and study later