Why is a probability wave required to describe an electron's location?
a. the electron's location can be precisely determined
b. electrons violate heisenberg's uncertainty principle.
c. the electron may be found at various distances from the nucleus.
d. the electron has less probability of being at the first bohr orbit than at any other distance.
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The probability wave is required to describe an electron's location so that the electron may be found at various distances from the nucleus.  

Option c

Explanation:

In quantum mechanics, the physical state of an electron can be described by its "wave function".

The standard probability interpretation states that the wave function of an electron is the probability amplitude and its modulus square which gives the probability density of finding an electron in a definite position in space.

The modulus square of the wave function not only gives us the probability density of the atom but it also tells about the possibility of finding an electron at the specific place. It gives us an idea about the distance of an electron from its nucleus. Hence, the probability wave is required to describe an "electron's location".

at positions a, g kinetic energy is maximum.

at position d, potential energy is maximum.

the old price per ounce is c/4.

the new price per ounce is c/3.6.

the ratio of the old price to the new one is

(c/4)/(c/3.6) = (c/c)×(3.6/4) = 0.9 . . = 9/10 . . "nine tenths" in either form