To review the characteristic reactions of acids and alkalis
To Planning a synthesis involves calculating how much of the reactants to mix together to make the amount of product required.
practise writing word and symbol equations.
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The PDF file contains MCQ (Multiple Choice Questions) related to Chemical Reactions and Equations. Chemical Reactions and Equations is the Chapter 1 of Class 10 Science (Chemistry).
Classic, mini chemistry experiments- some require materials typically found in a high school chemistry lab, while others are extremely simple. Very straightforward!
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MCQ on Chemical Reactions and Equations PDFAbdur Rohman
The PDF file contains MCQ (Multiple Choice Questions) related to Chemical Reactions and Equations. Chemical Reactions and Equations is the Chapter 1 of Class 10 Science (Chemistry).
Classic, mini chemistry experiments- some require materials typically found in a high school chemistry lab, while others are extremely simple. Very straightforward!
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Chemistry 201 Laboratory- Harold Washington College ReacJinElias52
Chemistry 201 Laboratory- Harold Washington College
Reactions of Copper and Percent Recovery
Introduction
In Chapter 4 of your textbook, we have covered the 3 main classes of reactions in aqueous
solution: precipitation reactions, acid-base reactions, and oxidation-reduction reactions. These
can be summarized as follows:
• In Precipitation reactions: a solid product forms from aqueous reactants. The product can
be predicted by using solubility rules.
• In Acid-base neutralization reactions: an acid (proton donor) reacts with a base (proton
acceptor) to form an ionic salt and sometimes water. You can recognize this type of
reaction by the presence of an acid and base in the reactants.
• In Oxidation-reduction reactions (or redox for short): electrons are transferred between
reactants. So you will always see changes in oxidation number within this type of
reaction.
In this lab, we will be examining these reactions by carrying out a sequence of reactions
starting from metallic copper in the form of a wire. According to the Law of Mass Conservation,
covered in section 2.3 of your textbook, mass is neither created nor destroyed. So since no
copper is added or removed during the course of these reactions, you should be able to
quantitatively recover all of the copper metal you started with at the end of these reactions (if
everything goes well).
You need to carefully observe and record your observations. You should be able to
carefully describe the reactions in terms of color change (color of solution or solid forming), gas
formation (as bubbles), heat generation (change in temperature), or precipitate formation,
throughout the experiment.
At the end of the reactions series, you will collect the copper recovered and calculate the
percent recovery (% yield) of copper using this formula:
% yield = actual amount of Cu recovered x 100 %
original amount of Cu
Materials and Equipment
• Piece of copper wire (about 0.5 g)
• concentrated HNO3 (aq)
• 3.0M NaOH
• 6.0M H2SO4
• solid zinc
• 2-250 mL beakers, 400 mL beaker
• 50 mL graduated cylinder
• boiling chips
• stirring rod
• iron ring and ring stand, wire gauze,
• Bunsen burner
• evaporating dish
• electronic balance
Chemistry 201 Laboratory- Harold Washington College
SAFETY NOTES
• Safety goggles should be worn at all times
• Sulfuric acid, nitric acid, and sodium hydroxide are corrosive chemicals and should be
handled with care.
• Gloves are to be worn when handling these chemicals.
• Waste should be put in the designated container in the hood. Never throw chemicals
down the drain.
PROCEDURE
1. Obtain a piece copper wire, measure its mass to the nearest 0.01 g, and place it in a 400
mL beaker.
2. IN THE HOOD, add 4-5 mL of concentrated nitric acid, HNO3, to the beaker. (Caution:
Be careful not to get any of the nitric acid on yourself. If you do, wash it o ...
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2. ACIDS AND ALKALIS AIMS: To review the characteristic reactions of acids To practise writing word and symbol equations.
3. Water sodium hydroxide hydrochloric acid sodium chloride Copy and link the symbols to their names
4. For any reaction, what you start with are called the reactants, and what you form are called the products. 1. The reactants are one molecule of Sodium ……………. and one molecule of ……………… acid 2. The products are one molecule of…………….. and one molecule of ………………. 3. Are all chemicals involved compounds or elements Complete the sentences below
5. Look at the equations above and explain the difference
6.
7. Acid reactions 1. acid + metal salt + hydrogen 2. acid + metal oxide salt + water 3. acid + metal carbonate salt + carbon dioxide + water Your Task UNDERSTAND THE RULES ABOVE FOR REACTION OF ACIDS WITH METALS, METAL OXIDES AND METAL CARBONATES
9. Acids with Metals Put about 5 cm3 of dilute acid in a test tube. Add a small piece of magnesium ribbon. If a gas forms, trap some by putting a finger over the end of the tube. After a while test the gas with a burning splint. What is your observation?
10. Acids with Metal oxides Put about 5 cm3 of dilute acid in a test tube. Add a small spatula measure of black copper oxide. Warm gently. Filter, collecting the filtrate in a test tube. Note the colour of the solution after filtering. Record your observations .
11. Acids with Metal carbonates Put about 5 cm3 of dilute acid in a test tube. Add a couple of marble chips (calcium carbonate). If a gas forms, use a delivery tube to bubble the gas through limewater in another test tube.
12. TASK Write word equations to describe the reactions of hydrochloric acid with magnesium, with copper oxide, and with sodium carbonate.
13. Answer True/False and explain your choice of answer 1. Chemists who synthesize new chemicals need knowledge of science explanations combined with practical skills. 2. It is important to understand how to control reactions so that they are neither too slow or dangerously fast. 3. Planning a synthesis involves calculating how much of the reactants to mix together to make the amount of product required.