Examples of concentration in the following topics:
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- Diluting a solution involves adding additional solvent to decrease the solution's concentration.
- Dilution refers to the process of adding additional solvent to a solution to decrease its concentration.
- Dilution can also be achieved by mixing a solution of higher concentration with an identical solution of lesser concentration.
- What is the final concentration of the diluted solution?
- As is evidenced in this example, the concentration is reduced by a factor of ten in each step.
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- The effect of changes in the concentration of products and reactants in a reversible reaction can be predicted by Le Chatelier's Principle.
- If a chemical system at equilibrium experiences a change in concentration, temperature, volume, or partial pressure, then the equilibrium shifts to counteract the imposed change.
- Changing the concentration of an ingredient will shift the equilibrium toward the side that reduces the concentration change.
- Suppose we were to increase the concentration of CO in the system.
- Evaluate how a change in concentration will affect a chemical equillibrium
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- Since we know what our Kc value is and the initial concentrations of reactants, we can set up an ICE chart to track the changes in concentration, as the reaction proceeds towards equilibrium.
- We can designate x as the change in concentration of N2 and O2.
- Knowing the initial concentration values and equilibrium constant we were able to calculate the equilibrium concentrations for N2, O2 and NO.
- The equilibrium concentration is the sum of the initial concentration and the change, which is derived from the reaction stoichiometry.
- Calculate the concentrations of reaction components at equilibrium given the starting concentrations and the equilibrium constant
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- Walther Nernst proposed a mathematical model to determine the effect of reactant concentration on the electrochemical cell potential.
- When reactant concentrations differ from standard conditions, the cell potential will deviate from the standard potential.
- In chemistry, a reaction quotient is a function of the activities or concentrations of the chemical species involved in a chemical reaction.
- Gibbs' key contribution was to formalize the understanding of the effect of reactant concentration on spontaneity.
- When a change in the concentration or activity of reactants occurs, or the temperature or pressure changes, the output voltage changes.
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- In chemistry, pH is a measure of the hydrogen ion (H+) concentration in a solution.
- The pH of a buffer can be calculated from the concentrations of the various components of the reaction.
- They consist of using the initial concentrations of reactants and products, the change they undergo during the reaction, and their equilibrium concentrations.
- ICE table for the buffer solution of NH4+ and NH3 with the starting concentrations.
- Describes the final concentration of the reactants and products at equilibrium.
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- A zero-order reaction has a constant rate that is independent of the concentration of the reactant(s); the rate law is simply $rate=k$ .
- As such, increasing or decreasing the concentration of the reacting species will not speed up or slow down the reaction rate.
- In the case of a zero-order reaction, the rate constant k will have units of concentration/time, such as M/s.
- [A]0 represents the initial concentration and k is the zero-order rate constant.
- Use graphs of zero-order rate equations to obtain the rate constant and the initial concentration data
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- A first-order reaction depends on the concentration of one reactant, and the rate law is: $r=-\frac{dA}{dt}=k[A]$ .
- A first-order reaction depends on the concentration of only one reactant.
- As usual, k is the rate constant, and must have units of concentration/time; in this case it has units of 1/s.
- To do this, we can measure an initial concentration of N2O5 in a flask, and record the rate at which the N2O5 decomposes.
- We can then run the reaction a second time, but with a different initial concentration of N2O5.
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- Reaction rates can be determined experimentally by measuring the concentration of a reactant and/or product over time.
- There are two main ways to measure the concentrations of reactions: by measuring the changes in an observable physical property, or by taking samples of the reaction solution and measuring concentration directly.
- Chemical methods yield concentrations directly.
- By Beer's law, the absorbance of the solution is directly proportional to the concentration of the C60O3 in solution, so observing the absorbance as a function of time is essentially the same as observing the concentration as a function of time.
- The absorbance is proportional to the concentration of the C60O3 in solution, so observing the absorbance as a function of time is essentially the same as observing the concentration as a function of time.
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- An acid-base titration is used to determine the unknown concentration of an acid or base by neutralizing it with an acid or base of known concentration.
- Using the stoichiometry of the reaction, the unknown concentration can be determined.
- The reactant of unknown concentration is deposited into an Erlenmeyer flask and is called the analyte.
- The other reactant of known concentration remains in a burette to be delivered during the reaction.
- Step 3: Calculate the molar concentration of HCL in the 25.00 mL sample.
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- This was done intentionally, because in order to determine the reaction order in A, we need to choose two experimental trials in which the initial concentration of A changes, but the initial concentration of B is constant, so that the concentration of B cancels.
- We do this by picking two trials in which the concentration of B changes, but the concentration of A does not.
- Note that both k and the concentrations of A cancel.
- A table showing data for three trials measuring the various rates of reaction as the initial concentrations of A and B are changed.