Which of the following is true about the properties of aqueous solutions? A pH c

Question

Which of the following is true about the properties of aqueous solutions? A pH change from 5.0 to 6.0 reflects an increase in hydroxide ion concentration ([OH^-]) of 20% A pH change from 8.0 to 6.0 reflects a decrease in the proton concentration ([H^+]) by a factor of 100 Charged molecules are generally insoluble in water Hydrogen bonds form readily in aqueous solutions the pH can be calculated by adding 7 to the value of the pOH. Which of the following statements about buffers is true? A buffer composed of a weak acid of p_ka = 5 is stronger at pH 4 than at pH 6 At PH values lower than the pK_a, the salt concentration is higher than that of the acid The pH of a buffered solution remains constant no matter how much acid or base is added to the solution The strongest buffers are those composed of strong acids and strong bases When p_H = pK_a, the weak acid and salt concentrations in a buffer are equal If the delta of the reaction A leftrightarrow B is -40 kJ/mol under standard conditions the reaction: is at equilibrium will never reach equilibrium will not occur spontaneously will proceed at a rapid rate will proceed spontaneously from left to right When a mixture of glucose 6-phosphate and fructose 6-phosphate is incubated with the enzyme phosphohexose isomerase (which catalyzes the interconversion of these two compounds) until equilibrium is reached, the final mixture contains twice as much glucose 6-phosphate as fructose 6-phosphate. Which one of the following statements is best applied to this reaction outlined below? (r = 8.315 J/mol K: T = 298 K) Glucose 6-phosphate leftrightarrow fructose 6-phosphate delta G degree is incalculably large and negative delta G degree is -1.72 KJ/mol delta G degree is zero delta G degree is zero delta G degree is +1.72 KJ/mol delta G degree is incalculably large and positive In glycolysis, fructose 1, 6-bisphosphate is converted to two products with a standard free-energy change (delta G degree) of 23.8 KJ/mol. Under what conditions encountered in a normal cell will the free-energy change(delta G) be negative, enabling the reaction to proceed spontaneously to the right? Under standard conditions, enough energy is released to drive the reaction to the right The reaction will not go to the right spontaneously under any conditions because the delta G degree is positive The reaction will proceed spontaneously to the right if there is a high concentration of products relative to the concentration of fructose 1, 6-bisphosphate The reaction will proceed spontaneously to the right if there is a high concentration of fructose 1, 6-bisphosphate relative to the concentration of products None of the above conditions is sufficient

Explanation / Answer

Ans 6. D Hydrogen bonds form readily in aqueous solutions.

Hydrogen bonds are formed in between hydrogen and any other atom such as nitrogen , oxygen or fluorine . Since aqueous solutions have water as the solvent medium , that has both hydrogen and oxygen atoms in its molecule , the development of dipoles becomes easier and hence the hydrogen bonds are formed readily.

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