During the course of the experiment, which of the following happens to the NO3- ions? They remain dissolved in the filtrate solution. M+ is an unknown metal cation with a 1+ charge. A student dissolves the chloride of the unknown metal, MCl, in water to make it 100.0 mL of solution.
A student combines the solutions pouring them into a larger, previously empty beaker Z and observes the formation of a white precipitate. Assuming that volumes are additive, which of the following sets of solutions could be represented by the diagram above?
Bronsted Lowry Acid-Base reaction Solid Al(NO3)3 is added to distilled water to produce a solution in which the concentration of nitrate, [NO3-], is .10M. What is the concentration of the aluminum ion, [Al3+], in this solution?
In a titration experiment, H2O2(aq) reacts with aqueous MnO4-(aq) as represented by the equation above. The dark purple KMnO4 solution is added from a buret to a colorless, acidified solution of H2O2(aq) in an Erlenmeyer flask.
Which cation would be predicted by Coulomb's law to have the strongest ion-dipole attraction to water, and why? Mg2+Mg2+ , because it has the largest charge-to-size ratio.
What effect will increasing [H+] at constant temp have on the reaction represented above? The frequency of collisions between H+(aq) ions and ClO- (aq) ions will increase.
Which of the following best helps to explain why the value of ΔH° for the dissolving of CaF2 in water is positive? Ca2+ ions have very strong ion-ion interactions with F- ions in the crystal lattice.
What happens to the temperature of the contents of the vessel as the reaction occurs? (A) The temperature must increase, because according to Le Châtelier's principle, an increase in temperature causes more products to form.
The overall concentration of hydrogen ions is inversely related to its pH and can be measured on the pH scale (Figure 1). Therefore, the more hydrogen ions present, the lower the pH; conversely, the fewer hydrogen ions, the higher the pH.
The number of hydrogen ions that the water will receive determines the pH. When a basic substance enters the water it will take up hydrogen ions. This will raise the pH of the water....Acids and bases.pHproduct0hydrochloric acid13 more rows
Real gas behaves like ideal gas at high temperature and low pressure.
Which of the following best describes the change that takes place immediately after the CH3OH(l) is introduced into the previously evacuated vessel? A physical change takes place because intermolecular attractions are overcome.
Which of the following is a correct scientific justification for spraying water on the blossoms to protect them from temperatures below −2°C−2°C? The freezing of water is an exothermic process; thus, water that freezes on the blossoms releases heat to keep the blossoms at or above −2°C−2°C.
If the concentration is doubled, the rate will quadruple (second order reaction). : rate = k. If the concentration is doubled, the rate will stay the same (zeroth order reaction).
The effect of increasing the temperature on a system at equilibrium can be summarized as follows: increasing the temperature increases the magnitude of the equilibrium constant for an endothermic reaction, decreases the equilibrium constant for an exothermic reaction, and has no effect on the equilibrium constant for a ...
The reaction will react as if a reactant or a product is being added and will act accordingly by shifting to the other side. For example, if the temperature is increased for an endothermic reaction, essentially a reactant is being added, so the equilibrium shifts toward products.
The value of pH is inversely related to the concentration of hydrogen ions. Hence, when we increase the concentration of H+ (aq) ions in a solution the pH of the solution decreases.
When a type of substance called a Bronsted acid dissolves in water, it releases hydrogen ions, increasing the hydrogen ion concentration in the liquid. Chemists classify the measure of hydrogen ion concentration as pH: the lower the pH, the higher the concentration of hydrogen ions.
AcidsAcids increase the number of hydrogen ions (H+) in a solution (there are more hydrogen ions than hydroxide ions) and the resulting solution is said to be acidic. Bases increase the number of hydroxide ions (there are more hydroxide ions than hydrogen ions) and the resulting solution is said to be basic or alkaline.
If an acid is added to the solution, hydronium ion concentration increases which increases the acidity of the solution. If any base is added, it has more hydroxide ions which increases the basicity of the solution and makes it more alkaline in nature.
d) Nitrogen atoms have a smaller nuclear charge than oxygen atoms
a) Nitrogen atoms have a half filled p subshell
Beaker X and Beaker Y each contain 1.0 L of solution, as shown above. A student combines the solutions pouring them into a larger, previously empty beaker Z and observes the formation of a white precipitate. Assuming that volumes are additive, which of the following sets of solutions could be represented by the diagram above?
The mass percent of carbon in pure glucose, C6H12O6, is 40 percent . A chemist analyzes an impure sample of glucose and determines that the mass percent of carbon is 38.2 percent. Which of the following impurities could amount for the low mass percent of carbon in the sample?
They remain dissolved in the filtrate solution.
The ions of Group III are precipitated as their sulfides, or as their hydroxides, from a basicsolution of hydrogen sulfide. The sulfides of the ions of Group III are not sufficiently insolubleto be precipitated in the acidic solution of hydrogen sulfide of Group II but will be precipitatedby basic solutions of hydrogen sulfide.
The ions of Groups II and Groups III are separated by precipitation of their insoluble sulfides.The sulfide ion is furnished by the weak electrolyte gaseous hydrogen sulfide, which is onlysparingly soluble in water. At 25˚C and 1 atmosphere pressure, a saturated aqueous solutioncontains about 0.1 mole in a liter.)
After adding a reagent, stir the solution thoroughly before drawing any final conclusions.This should be done whether the reaction is carried out in a centrifug e tube or a casserole.Often additional quantities of the reagent must then be added so that an excess is present.