chemical_detective_lab

You have an unknown solution and you want to determine if it contains ammonia. How will you detect its presence in the laboratory analysis? Please provide two ways to analyze its presence and explain your chosen technique in determining the ammonia.

Use the solubility generalizations on the information page to predict if one or more precipitates will form when aqueous solutions of sodium acetate (NaCH3COO) and potassium hydroxide (KOH) are mixed. Write the formula of any precipitate that could form in one of the boxes. If a box is not needed, leave it blank. If no precipitate is predicted, leave both boxes blank.

Could someone please help! No plagiarism, please! Could someone please help me with this! What is in the image is what I have been able to get done so far No Plagiarism Please!

How can we answer these questions on solution stoichiometry and equilibrium?

4. Write the Molecular, Complete lonic and Net lonic equations for following reaction. Ammonium bromide and lead (11) nitrate react to form lead (II) bromide and ammonium nitrate. 5. You need to selectively precipitate and separate the metal ions Co*, Pb*?, and Sr2 in a tap water sample. This means you need to precipitate out each heavy metal in the sample separately so that only one type of heavy metal is removed by precipitation at a time. The only solutions available for you to precipitate the metals are aqueous solutions of NaCl, Na,SO, and NaOH. Write the balanced net ionic equation for each precipitation reaction (1 net ionic for each metal ion) IN THE ORDER they must be precipitated. First: Second: Third:

QUESTION #1: TOPIC: Solving for a reactant in solution  One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe(s) +CuSO4(aq) →Cu(s) +FeSO4(aq) Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 350. mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 93. mg. Calculate the original concentration of copper(II) sulfate in the sample. Round your answer to 2 significant digits.   ? g/L         QUESTION#2: TOPIC: Limiting reactants…

Your lab assignment presentation involves putting together a presentation to show other students on how to perform titration. In other words, your presentation can be used to show other students (next term) how they can perform a titration by following your instructions and calculations. To do this presentation, we are giving you the type of acid, acetic acid, the type of base, NaOH to be used, and you will use phenolphthalein as the indicator. You will use the data given to you to be used as an example of how to solve the mathematical calculations. At the end of your presentation, you will show the unknown concentration of the acetic acid (Molarity) and will also show the % mass/ vol of the Vinegar solution. Part 1 Purpose of a titration, what is titration and why do we perform a titration? Instrumentation- what are the instruments, glassware used when performing a titration. Chemicals and Procedures. What chemicals are needed? List and explain the procedures for this experiment.…

This is the data for questions 15 through 18: Volume of Volume of Volume of water, В, Volume of Time from mixing to dramatic color A, C, change, sec ml ml ml ml 1.0 1.0 2.0 96.0 4 1.0 3.0 2.0 94.0 4 15) Which reactant concentration have we changed? a) A b) B c) C d) no reactant concentrations changed 16) What was the change in concentration of that reactant? a) no change b) doubled c) tripled d) increased by the power of 10

Scoring: Your score will be based on the number of correct matches minus the number of incorrect matches. There is no penalty for missing matches. Use the References to access important values if needed for this question. Each of the insoluble salts below are put into 0.10 M hydrobromic acid solution. Do you expect their solubility to be more, less, or about the same as in a pure water solution ? magnesium fluoride calcium sulfite silver bromide Submit Answer Clear All More soluble than in pure water. Similar solubility as in pure water. Less soluble than in pure water. Retry Entire Group 5 more group attempts remaining

O Kf will change depending on what solute is dissolved in the solvent. QUESTION 11 Which term can be used to describe the process in the reaction below? 2 NaHCO3 (s) Na2CO3 (s) + H2O (g) + CO2 (g) Dissociation Precipitation Hydration Decomposition QUESTION 12 Which of the following would NOT be considered valid sources of error in a laboratory experiment? Click Save and Submit to save and submit. Cick Suve All Answers to save all ansicers

PrecipAa

In an acid-base reaction, a strong acid will form a weak base. True False

Volumetric Analysis Liza carefully pipets 25.0 mL of 0.525 M NaOH into a test tube. She places the test tube into a small beaker to keep it from spilling and then pipets 75.0 mL of 0.355 M HCl into another test tube. When Liza reaches to put this test tube of acid into the beaker along with test tube of base, she accidentally knocks the test tubes together hard enough to break them and their respective contents combine in the bottom of the beaker. Is the solution formed from the contents of the two test tubes acidic or basic? What is the pH of the resulting solution?

You dilute the river water 10 times for the analysis of SDS concentration. The instrument measures an average molar concentration of SDS in the diluted river water to be 1.689 10-4 mol/L. The molar mass of SDS is 288.4 g/mol. What is the mass concentration of SDS in the original river water? 4.87 10-1 g/L 4.87 102 g/L 5.86 106 g/L 5.86 10-5 g/L

Can someone please help complete the blank table below?

In this experiment, you will be running multiple trials, each with a TOTAL volume of 35 mL, but with an increasing the amount of vinegar in that mixture each time. What you think will happen as you go from trial 1 all the way through trial 8? The highest amount of NaHCO3 will react in trial #1. The highest amount of NaHCO3 will react in trial #8. The amount of NaHCO3 will react more and more with each trial until a certain point, at which it doesn't matter how much vinegar is added because all of the NaHCO3 will be used up. The amount of NaHCO3 will react less and less with each trial until a certain point, at which it doesn't matter how much vinegar is added because all of the vinegar will be used up.

Complete the data below. H2SO4 concentration was 1.304 M. Na2B4O7·10 H2O concentration was 0.105 M.

2. For his second experiment, Samuel uses vinegar instead of acetic acid powder. He sets up three experimental trials with different reaction conditions. He records all his data in the table below for the three trials. Trial Mass of Baking Soda (g) Temperature (°C) Volume of Vinegar (ml) Reaction time to completion (s) 1 10.0 25.0 60.0 41 2 10.0 40.0 60.0 23 3 10.0 55.0 60.0 12 b) Explain the reason for the pattern in Samuel's results. Your explanation should refer to what is happening between the reactant particles. BIUE E mR E ca7.020 26 i Aa 2048 MacBook Air 80 888 DII F11 F4 FS F2 F3 & %23 2$ dele 3 4 7 8 { Y P W E R S D F G H J K > V B M. %3D command option command - - V - N