"Configuration of Sodium Chloride Solution with Certain Solute Mass Fraction" Solution PPT Courseware

Description

"Configuration of Sodium Chloride Solution with Certain Solute Mass Fraction" Solution PPT Courseware

Knowledge review:

Solution consists of solute and solvent,

Mass of solution = Mass of solute + Mass of solvent = Volume of solution × Density of solution

Mass fraction of solute = mass of solute/mass of solution × 100%

Experimental Activity 1: Prepare 50g of 6% NaCl solution

1Experimental steps:

(1) Calculation: NaCl mass = 50g × 6% = 3g, H2O mass = 50g-3g = 47g.

(2) Weighing: Weigh 3gNaCl on a pallet balance, and measure 47mlH2o with a graduated cylinder.

(3) Dissolution: Stir with a glass rod to dissolve NaCl.

(4) Bottle: Put the solution into a narrow-mouth bottle and label it (indicate the concentration and solution name: 6% NaCl solution).

2 main instruments:

Pallet balance, medicine spoon, measuring cylinder, plastic tip dropper, glass rod, narrow-mouth bottle

3 Error analysis

For example: When a student was nervous and poured the water from the measuring cylinder into the beaker, and accidentally splashed it outside the beaker, the mass fraction of the obtained sodium chloride solution would be ____.

Analysis: Mass fraction of solute = solute mass / solute mass + solvent mass × 100%

The mass of the solvent becomes smaller and the mass fraction of the solute becomes larger.

1 When pouring the sodium chloride solid into the beaker, some of the sodium chloride solid remains on the paper, then the mass fraction of the obtained sodium chloride solution is _____.

Analysis: The mass of the solute becomes smaller, and the mass fraction of the solute becomes smaller.

2. When measuring water, look up and read. Then the solute mass fraction of the solution obtained is _____.

Analysis: Looking up at the reading, the mass of the solvent becomes larger and the mass fraction of the solute becomes smaller.

The main cause of experimental errors is: changes in solute and solvent mass

⑴Possible reasons for the actual value to be too small

① The amount of solute dissolved has decreased: the solute itself is impure; the left and right objects are weighed; the solute is scattered; the solute is bottled and stored before it is completely dissolved.

② The amount of solvent has increased: look up and measure; there is water on the inner wall of the beaker; there is water on the inner wall of the reagent bottle

⑵ Possible reasons for the actual value to be too large

①The amount of solvent is reduced: measure the solvent while looking down; the measured water is not completely transferred to the beaker

② The amount of dissolved solute increases: when weighing, the weights used are rusty or stained with oil.

Experimental Activity 2: Use 6% NaCl solution to prepare 50g of 3% NaCl solution

Concentrate solution by adding water to make dilute solution.

(The mass of the solute remains unchanged)

25g of 6% NaCl solution (density of 1.04g/ml) and 25g of water are required.

1 Experimental steps:

(1) Calculation: Volume of 6% NaCl solution = ,

(2) Measurement: Use a graduated cylinder to measure the 6% NaCl solution and water respectively.

(3) Dissolution: Mix the solution evenly.

(4) Bottle: Put the solution into a narrow-mouth bottle and label it.

2 main instruments:

Beakers, measuring cylinders, droppers, glass rods, narrow-mouth bottles.

2 When preparing a sodium chloride solution with a certain mass fraction, the following operational errors will cause the solute mass fraction of the prepared solution to decrease ( )

A. When weighing sodium chloride with a pallet balance, place the weight on the left pan but do not use the balance.

B. When measuring distilled water with a graduated cylinder, look up at the lowest point of the concave liquid surface.

C. When pouring the water from the measuring cylinder into the beaker, water spilled out

D. When transferring the prepared sodium chloride solution to a narrow-mouth bottle, part of the solution was accidentally spilled

3 To prepare 100g of sodium chloride solution with a solute mass fraction of 10%, the following operations are correct ( )

A. Place 10g of sodium chloride solid directly on the tray of the balance and weigh it

B. When measuring 90ml of water, read from above

C. To speed up the dissolution of the solid, stir the solution with a thermometer

D. Pour the prepared solution into the narrow-mouth bottle, cap the bottle tightly and label it

Class summary:

Prepare a solution with a certain solute mass fraction:

Steps: 1 Calculate 2 Weigh 3 Dissolve 4 Bottle

Instruments: medicine spoon, pallet balance, measuring cylinder, rubber dropper, beaker, glass rod, narrow-mouth bottle

Error analysis: the impact of changes in solute mass and solvent mass on the results

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"Configuration of Sodium Chloride Solution with Certain Solute Mass Fraction" Solution PPT Courseware 3:

"Configuration of Sodium Chloride Solution with Certain Solute Mass Fraction" Solution PPT Courseware 3 Learning Objectives 1. Simple calculations related to solute mass fractions are performed. 2. A solution with a certain solute mass fraction will be prepared. Key Points and Difficulties Key Points: The operating steps and basics of preparing solutions..

"Configuration of Sodium Chloride Solution with Certain Solute Mass Fraction" Solution PPT Courseware 2:

"Preparation of Sodium Chloride Solution with Certain Solute Mass Fraction" Solution PPT Courseware 2 [Pre-class Test] 1. Mass fraction of solute =---------100% 2. When preparing 50g of 6% NaCl solution: (1) After calculation, weigh ____gNaCl on ____ and pour it into a dry and clean...

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Update Time: 2024-07-01

This template belongs to Chemistry courseware People's Education Press Ninth Grade Chemistry Volume 2 industry PPT template

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