C5 Precipitation
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When sodium carbonate solution and calcium chloride solution are mixed, a precipitation reaction occurs where calcium carbonate forms as an insoluble solid precipitate. The chemical equation is: sodium carbonate + calcium chloride → sodium chloride + calcium carbonate (s). Calcium carbonate is the precipitate that forms.
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value is $24.000 for an interest rate of 7%. ?? 4A
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24,000 or, A = $ 2,091.40 Thus, Value of A $ 2,091.40.
The role of the ion product
Adding AgNO3 to a saturated solution of AgCl increases the concentration of Ag+ ions, making the ion product (Qsp) greater than the solubility product (Ksp) and causing the solution to be out of equilibrium. The solution will re-equilibrate by precipitating excess AgCl, resulting in a higher Ag+ concentration than Cl- concentration. Similarly, adding NaCl increases the Cl- concentration, making Qsp > Ksp and causing re-equilibration with a lower Ag+ concentration than Cl-. The concentrations of ions in equilibrium solutions fall along a curved line where the ion product equals Ksp.
CLASS X CHEMISTRY
This document discusses acids, bases, and salts. It provides information on baking powder and its main ingredients, why acid should be diluted by adding it to water, how the pH of milk changes when it turns to curd, properties and uses of washing soda, and classifications of common acids and bases as strong or weak. Key points covered include that baking powder contains sodium bicarbonate and tartaric acid which react to produce carbon dioxide and make bread fluffy, adding acid to water is safer than water to acid due to exothermic reactions, and milk curdling increases acidity as shown by lower pH due to lactic acid formation.
Sodium bicarbonate (Na+HCO3- ) is mildly alkaline.pdf
Sodium bicarbonate (Na+HCO3- ) is mildly alkaline and it reacts withacids: H+ +
HCO3- =H2CO3 (carbonic acid) which is unstable inwater and breaks down into water &
Carbon Dioxide : H2CO3(aq) --> H2O(l) + CO2 (g) . Inan open container at atmospheric
pressure, the CO2 escapes, so thereaction is irreversible. Alka Seltzer must contain some
mildacid in solid form, maybe acetylsalicylic acid (aspirin). When placed in water, the acid and
bicarbonate react and fizz(CO2). Bicarbonate is useful in antacids for the same reason- stomach
acid (HCl) reacts with the bicarbonate producing waterand carbon dioxide. The carbon dioxide
leaves (burp!) andonly water remains where there once was a strong acid.
Solution
Sodium bicarbonate (Na+HCO3- ) is mildly alkaline and it reacts withacids: H+ +
HCO3- =H2CO3 (carbonic acid) which is unstable inwater and breaks down into water &
Carbon Dioxide : H2CO3(aq) --> H2O(l) + CO2 (g) . Inan open container at atmospheric
pressure, the CO2 escapes, so thereaction is irreversible. Alka Seltzer must contain some
mildacid in solid form, maybe acetylsalicylic acid (aspirin). When placed in water, the acid and
bicarbonate react and fizz(CO2). Bicarbonate is useful in antacids for the same reason- stomach
acid (HCl) reacts with the bicarbonate producing waterand carbon dioxide. The carbon dioxide
leaves (burp!) andonly water remains where there once was a strong acid..
Chapter Four Lecture
This document discusses various topics relating to solutions and solution chemistry, including:
- Solutions are homogeneous mixtures of two or more pure substances, with the solvent present in greatest abundance.
- When an ionic substance dissolves in water, the solvent pulls the individual ions from the crystal and solvates them, in a process called dissociation.
- Substances that produce ions when dissolved in water are called electrolytes, while nonelectrolytes may dissolve but do not produce ions. Soluble ionic compounds tend to be electrolytes.
- Strong electrolytes dissociate completely in water, while weak electrolytes only partially dissociate. Strong acids, bases, and soluble ionic
15saltspp.ppt
This document is a guide about acids, bases, and salts for A-level chemistry students. It covers topics like Brønsted-Lowry theory of acids and bases, strong and weak acids, alkalis, and reactions of hydrochloric acid with different substances. The guide explains key concepts and provides examples to help students understand the subject matter required by various examination boards. It is intended to be used for both classroom teaching and individual student revision.
Precipitation Titrations
1. Precipitation titrations involve the titration of an analyte solution with a reagent that causes the formation of an insoluble precipitate.
2. The Mohr method is commonly used for chloride determination and involves titrating a chloride solution with silver nitrate using potassium chromate as an indicator.
3. At the endpoint, excess silver nitrate reacts with potassium chromate to form a reddish brown silver chromate precipitate, indicating that all the chloride ions have been precipitated out as silver chloride.
Chemistry Equilibrium
This document discusses acid-base equilibria and solubility equilibria. It covers the common ion effect and how it impacts equilibrium, buffer solutions, acid-base titrations and indicators, solubility equilibria including Ksp expressions and calculations, and the effects of pH and common ions on solubility. It also briefly mentions complex ion equilibria.
Acidbasetitr
This document discusses acid-base titrations and summarizes the key steps in standardizing a sodium hydroxide (NaOH) solution and using it to determine the concentration of acetic acid in vinegar. It explains that NaOH is hygroscopic and absorbs moisture, so it must be standardized against a primary standard, potassium hydrogen phthalate (KHP), through titration. The standardized NaOH solution can then be used to titrate vinegar against it and calculate the moles and molarity of acetic acid present. It also discusses concepts like the pH at the equivalence point of a titration involving a weak acid and strong base.
Acidbasetitr 150602233035-lva1-app6891
This document discusses acid-base titrations and summarizes the key steps in standardizing a sodium hydroxide (NaOH) solution and using it to determine the concentration of acetic acid in vinegar. It explains that NaOH is hygroscopic and absorbs moisture, so it must be standardized against a primary standard, potassium hydrogen phthalate (KHP), through titration. The standardized NaOH solution can then be used to titrate vinegar against it and calculate the moles and molarity of acetic acid present. It also discusses concepts like the pH at the equivalence point of a titration involving a weak acid and strong base.
Carbon and compounds
Diamond has a giant covalent structure where each carbon atom is bonded to four other carbons, giving it properties like hardness and electrical insulation. It is used in cutting, jewelry due to its brilliance, and lasers. Graphite has layers of hexagonal carbon sheets bonded by van der Waals forces, making it soft and a conductor. It is used as a lubricant, in electrodes, and pencils. Hard water contains calcium and magnesium ions that form precipitates with soap. Temporary hardness can be removed by boiling or adding washing soda while permanent hardness requires ion exchange or distillation. Carbon forms oxides, is a reducing agent, and is important in combustion, fermentation, and the carbon cycle.
Ch4z5ereactions 110115225323-phpapp01
1) Aqueous solutions are homogeneous mixtures where a solute is dissolved in a solvent, usually water. Water is a good solvent due to its polar molecular structure.
2) Solutions can be strong or weak electrolytes depending on how completely the solute dissociates into ions when dissolved. Strong electrolytes fully dissociate into many ions, while weak electrolytes only partially dissociate.
3) Precipitation reactions occur when oppositely charged ions in aqueous solutions combine to form an insoluble ionic compound as a solid precipitate. These reactions can be used to separate out desired products through filtration.
Chemical equations best
1. The document discusses chemical equations, including word equations, balanced equations, and how to interpret and balance chemical equations.
2. It explains the key parts of a chemical equation including reactants, products, phases (solid, liquid, gas), and how to write ionic equations.
3. The document also covers different types of chemical reactions like synthesis, decomposition, single replacement, and double replacement reactions and how to predict products.
Chemistry M2 Acids bases salts
Acids provide H+ ions in water, while bases provide OH- ions. Examples of acids include HCl and H2SO4, while examples of bases include NaOH and KOH. When acids and bases react, they undergo a neutralization reaction producing water and a salt. For example, HCl + NaOH produces H2O + NaCl. Strong acids and bases fully dissociate in water, while weak ones only partially dissociate.
Lab tests ok1294990656
The document discusses several chemistry concepts and experiments including:
1) Testing for carbon dioxide by adding acid to carbonates which produces carbon dioxide gas.
2) Using flame tests to identify metal ions based on the color of flames they produce.
3) Metal ions forming precipitates when sodium hydroxide is added, such as calcium ions forming calcium hydroxide.
4) Experiments to test for chloride, sulfate, ammonium, nitrate, bromide and iodide ions using chemical reactions and indicators.
Chemistry edexcel as unit 1 chapter 1 chemical quantities_v0.03
Here are the key steps and observations from the experiment:
- Weigh out 0.56g of iron powder, which is 0.01 moles
- Add to excess copper(II) sulfate solution
- A displacement reaction occurs, producing copper metal
- Filter, wash, dry the copper product
- Weigh the copper produced
- If equation 1 is correct, the mass of copper should be 0.63g (0.01 moles of Cu)
- However, the actual mass obtained is higher, indicating equation 2 is correct
- Equation 2 involves a change in oxidation state of iron from 0 to +3, a redox reaction
So in summary, the experiment shows the reaction involves a redo
Bitsat previous-year-question-papers-2013
This document contains chemistry questions and answers related to various topics like periodic trends, Bohr model, oxidation states, organic reactions, acid-base properties, and electrochemistry. The questions test understanding of fundamental concepts and ability to apply trends and principles to solve problems. In summary:
- The questions cover a wide range of chemistry topics and require recalling definitions, concepts, and trends to select the right answer.
- Multiple choice questions have a single correct answer that can be arrived at by applying principles like periodic trends, acid-base properties, and knowledge of reaction mechanisms.
- The document serves as a self-assessment tool for students to evaluate their understanding of core chemistry concepts and ability to apply reasoning to
Ch7_PowerPoint_7.5 to 7.7.pdf
1) Water is a polar molecule due to the unequal sharing of electrons between the oxygen and hydrogen atoms. This gives water a partial negative charge on the oxygen side and partial positive charges on the hydrogen sides.
2) When ionic compounds dissolve in water, they dissociate into their constituent ions. The ions are then able to move freely within the water, allowing the solution to conduct electricity and making them electrolytes.
3) Double displacement precipitation reactions occur when two aqueous ionic solutions are mixed. The cations and anions are swapped between the reactants to form new ionic compounds. One of the products may have limited solubility and precipitate out of solution as an insoluble solid.
Reactions in aqeous solutions
Grade 10 Physical Sciences
Based on Andries Oliviers' CAPS aligned textbook
Focus area: Reactions in aqueous solutions
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C5 Precipitation
- 1. Precipitation A reaction is which a solid (precipitate) is formed. Objective: What you need to know is how to work out which chemical is the precipitate/the solid.
- 2. Question When sodium carbonate solution is mixed with calcium chloride solution, a precipitate is formed. What is it? Calcium chloride
- 3. Step 1: Write out the word equation When sodium carbonate solution is mixed with calcium chloride solution, a precipitate is formed. What is it? sodium carbonate + calcium chloride sodium chloride + calcium carbonate Explanations: When the solutions are mixed, the ions swap partner (displacement). AB + CD AD + BC
- 4. Step 2: Add state symbols When sodium carbonate solution is mixed with calcium chloride solution, a precipitate is formed. What is it? sodium carbonate + calcium chloride sodium chloride + calcium carbonate (aq) (aq) (aq) (s) Explanations: Use the solubility data from the table above. • Sodium carbonate (aqueous) – soluble in water therefore will remain dissolved • Calcium carbonate (solid) – insoluble in water therefore will be seen as a solid
- 5. Answer When sodium carbonate solution is mixed with calcium chloride solution, a precipitate is formed. What is it? sodium carbonate + calcium chloride sodium chloride + calcium carbonate (aq) (aq) (aq) (s) The precipitate formed is calcium carbonate (white solid). Calcium chloride