Entalphyofsolutionspart2 121121135409-phpapp02
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This document discusses the enthalpy of neutralization reaction between acids and bases. It defines enthalpy of neutralization as the energy released per mole of water formed in an acid-base reaction, which is an exothermic property. The reaction of a strong acid with a strong base produces water and heat. The procedures describe mixing two acid-base pairs, HCl with NaOH and HNO3 with NaOH, and measuring the temperature change to determine the enthalpy change of neutralization. Safety precautions for handling the acids and bases are also outlined.
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Entalphy of solutions part2
This document discusses the enthalpy of neutralization reaction between acids and bases. It defines enthalpy of neutralization as the energy released per mole of water formed in an acid-base reaction, which is an exothermic property. The reaction of a strong acid with a strong base produces water and heat. It then provides step-by-step instructions for experimentally determining the enthalpy change of two acid-base neutralization reactions: HCl + NaOH and HNO3 + NaOH.
Entalphy of solutions part2
This document discusses the enthalpy of neutralization reaction between acids and bases. It states that the enthalpy of neutralization is the energy released per mole of water formed in an acid-base reaction, which is an exothermic property. When a strong acid reacts with a strong base, water and heat are produced in an exothermic reaction. The experiments described involve measuring the temperature change when hydrochloric acid and nitric acid each react separately with sodium hydroxide to determine the enthalpy change.
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This document discusses classifying chemical reactions based on several factors:
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2. Whether heat is evolved or absorbed in the reaction.
3. The degree of oxidation of elements in reactants vs products.
4. The number and composition of reactants and products.
Students are asked to get into groups and classify sample chemical reactions according to these factors, then perform sample reactions demonstrating synthesis, decomposition, double replacement, and single replacement reactions.
Determination of enthalpy of neutralization of hydrochloric acid with sodium ...
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The heat of neutralization is heat produced when 1 mole of water is produced by the reaction of the acid and base
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Hess's law allows you to calculate the heat of reaction indirectly by adding together thermochemical equations with known heats of reaction to obtain the heat of reaction for a new equation. You can also use standard heats of formation, which are the changes in enthalpy accompanying the formation of one mole of a compound from its elements under standard conditions, to calculate heats of reaction for reactions at standard conditions. The document provides an example of using standard heats of formation to calculate the heat of reaction for the equation NH3(g) + HCl(g) → NH4Cl(s).
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- The heat absorbed during vaporization of a liquid is the same as the heat released during condensation of the vapor, known as the molar heat of vaporization and condensation.
- Heat is either absorbed or released when a solution forms, known as the molar heat of solution.
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Entalphy of solutions part2
This document discusses the enthalpy of neutralization reaction between acids and bases. It defines enthalpy of neutralization as the energy released per mole of water formed in an acid-base reaction, which is an exothermic property. The reaction of a strong acid with a strong base produces water and heat. It then provides step-by-step instructions for experimentally determining the enthalpy change of two acid-base neutralization reactions: HCl + NaOH and HNO3 + NaOH.
Entalphy of solutions part2
This document discusses the enthalpy of neutralization reaction between acids and bases. It states that the enthalpy of neutralization is the energy released per mole of water formed in an acid-base reaction, which is an exothermic property. When a strong acid reacts with a strong base, water and heat are produced in an exothermic reaction. The experiments described involve measuring the temperature change when hydrochloric acid and nitric acid each react separately with sodium hydroxide to determine the enthalpy change.
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Hess's law allows you to calculate the heat of reaction indirectly by adding together thermochemical equations with known heats of reaction to obtain the heat of reaction for a new equation. You can also use standard heats of formation, which are the changes in enthalpy accompanying the formation of one mole of a compound from its elements under standard conditions, to calculate heats of reaction for reactions at standard conditions. The document provides an example of using standard heats of formation to calculate the heat of reaction for the equation NH3(g) + HCl(g) → NH4Cl(s).
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The document discusses different types of heat transfer that occur during phase changes of matter:
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The document discusses chemical reactions and equations. It defines a chemical reaction as a process involving a chemical change where new substances are formed. A chemical equation is used to represent chemical reactions, showing reactants on the left and products on the right. There are five main types of chemical reactions: combination, decomposition, displacement, double displacement, and redox reactions. Redox reactions involve the gain or loss of oxygen or hydrogen through oxidation and reduction.
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The document discusses various topics related to acids and bases:
1. It defines acids and bases, and classifies common substances as acidic, basic, or neutral based on their hydrogen ion concentration in water. Examples of strong acids and bases are provided.
2. Indicators and their uses are described, including litmus, phenolphthalein, methyl orange, and bromothymol blue. Everyday uses include testing soil pH and swimming pool chemistry.
3. Acidic oxides such as SO2, SO3, and CO2 are identified, and their position in the periodic table is linked to their acidity. Most transition metal oxides are basic.
The Acidic Environment
The document discusses various topics related to acids and bases:
1. It defines acids and bases, and classifies common substances as acidic, basic, or neutral based on their hydrogen ion concentration in water. Examples of strong acids and bases are provided.
2. Indicators and their uses are described, including litmus, phenolphthalein, methyl orange, and bromothymol blue. Everyday uses include testing soil pH and swimming pool chemistry.
3. Acidic oxides such as SO2, SO3, and CO2 are identified, and their position in the periodic table is linked to their acidity. Most transition metal oxides are basic.
The acidic environment
The document discusses acids and bases. It defines acids as proton donors and bases as proton acceptors according to the Bronsted-Lowry theory. Strong acids completely ionize in water while weak acids only partially ionize, reaching an equilibrium between intact molecules and ions. The pH scale measures the concentration of hydrogen ions [H+], with lower pH indicating higher [H+] and higher acidity. Common strong acids include hydrochloric acid while acetic and citric acids are weak. A change in pH of 1 represents a ten-fold change in [H+]. The historical development of acid theories from Lavoisier to Arrhenius and Bronsted-Lowry is also outlined.
Biol101 chp3-pp-fall10-100919154932-phpapp01
This document summarizes key aspects of water and its importance for life on Earth from Chapter 3 of General Biology I. It discusses how water is essential for all living organisms and is the reason Earth is habitable. Water has unique physical and chemical properties, such as being a polar molecule, having high specific heat, and being an excellent solvent, that help moderate temperatures and support biochemical reactions in organisms. The document also describes how human activities like burning fossil fuels are increasing ocean acidification and acid rain, threatening aquatic ecosystems by interfering with processes like calcification.
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This document provides an overview of astronomy and the scientific method. It discusses:
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This document discusses the spectral classification of stars. It explains that the advent of the spectroscope in the 1800s allowed astronomers to classify stars according to their spectral similarities. Originally there were 26 classes, but now there are 7 major classes - O, B, A, F, G, K, M - representing decreasing temperatures from 30,000 K to 3,000 K. Three problems are presented: 1) sorting 5 stellar spectra by closest match to standard spectra, 2) noting how spectral lines change with temperature, and 3) identifying which spectral types are missing from the sample.
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- 1. ENTHALPY (HEAT) OF NEUTRALIZATION OF AN ACID-BASE REACTION By : Dr. Robert D. Craig, Ph.D. Enthalpy of neutralization: energy released per mole of water formed in an acid-base reaction – an “exothermic” property
- 2. ENTHALPY (HEAT) OF NEUTRALIZATION OF AN ACID-BASE REACTION Enthalpy of neutralization: energy released per mole of water formed in an acid-base reaction –an “exothermic” property The negative sign is a result of the heat which is lost by the system to the surroundings The reaction of a strong acid with a strong base is a exothermic reaction that produces water and heat as products
- 3. These acids are dangerous
- 4. ENTHALPY (HEAT) OF NEUTRALIZATION OF AN ACID-BASE REACTION H3O+ (aq) + OH- (aq) 2 H2O (l) + heat
- 5. Secondary caution as well • Acid to the Water! • Why add the acid to the water? Because the same general concept described above applies when you're mixing an acid or a base to water. A base is the opposite of an acid and they are corrosive for different reasons
- 6. ENTHALPY (HEAT) OF NEUTRALIZATION OF AN ACID-BASE REACTION Enthalpy change, DHn = -specific heat (H20) x combined massed (Acid - Base) x DT (H20)
- 7. This will be done for two acids Page 296 see data sheet HCl + NaOH HNO3 + NaOH
- 8. Acid base pair number one • HCl + NaOH Clean two 250 mL Erlenmeyer flasks with soap, then rinse and drain. Repeat this until they drain cleanly without leaving droplets adhering to the sides, using purified water for a final rinse.
- 9. pair number one • Clean and dry the calorimeter with a towel. Make sure it doesn't leak. From the solutions available in the laboratory, rinse one of the Erlenmeyer flasks with a few mL of 0.500 M HCl and then drain. Rinse the other flask with a few mL of 0.500 M NaOH and drain. Label the flasks to avoid confusion
- 10. Becareful!!!!!!!50x • To obtain an accurate temperature measurement, it is essential that the thermometer bulb be completely emersed in the solution. If reaching thermal equilibration takes a long time, you may wish to dry off the thermometer and recheck the acid temperature before the final mix
- 11. Be careful!!!! 50x • If the two temperatures differ a bit before mixing, take the initial mixed solution temperature to be the average of the acid and base temperatures. Finally, carefully pour the base into the acid, stir gently with the thermometer, and record the exact time of mixing.
- 12. Acid base pair number two • HNO3 + NaOH • Please redo the same procedure as you did for • HCl + NaOH •
- 13. Last sentence • Enthalpy change, DHn is generally expressed in units of kJ/mol of water that forms from the reaction. • The mass (grams) of the solution equal the combined masses of the acid and base solution (this is important!!!!)