Holooly Plus Logo
Holooly Plus Logo

Question 8.1: Divide: 6.4 * 10^8 / 2.57 * 10^10

\text { Divide: } \frac{6.4 \times 10^{8}}{2.57 \times 10^{10}}
The Blue Check Mark means that this solution has been answered and checked by an expert. This guarantees that the final answer is accurate.
Learn more on how we answer questions.
6.4 \div 2.57=2.5

 

Subtract exponents:

 

10^{8} \div 10^{10}=10^{8-10}=10^{-2}

 

Answer:

 

2.5 \times 10^{-2}

Related Answered Questions

Buffer pH Calculation What is the pH of a solution if you mix 100 mL of 0.2 M HEPES in the acid form with 200 mL of 0.2 M HEPES in the basic form? Strategy To use the Henderson-Hasselbalch equation, you need the ratio of the conjugate base to weak acid forms of the buffer. Since the HEPES solutions

Verified Answer:
First we must find the p K_{ a }, w...

Acid Strength Which is the stronger acid: (a) Benzoic acid with a Ka of 6.5 * 10^-5 or hydrocyanic acid with a Ka of 4.9 * 10^-10? (b) Boric acid with a pKa of 9.14 or carbonic acid with a pKa of 6.37? Strategy Relative acid strength is determined by comparing the Ka values or the pKa values. If

Verified Answer:
(a) Benzoic acid is the stronger acid; it has the ...

Water Equation The [OH^-] of an aqueous solution is 1.0 * 10^-4 M. What is its [H*O^+]? Strategy To determine the hydrogen ion concentration when you know the hydroxide ion concentration, you simply divide the [OH^-] into 10^-14.

Verified Answer:
We substitute into the equation:   \be...

Calculating pH (a) The [H3O^+] of a certain liquid detergent is 1.4 * 10^-9 M. What is its pH? Is this solution acidic, basic, or neutral? (b) The pH of black coffee is 5.3. What is its [H3O^+]? Is it acidic, basic, or neutral? Strategy To determine the pH when given the concentration of a hydrogen

Verified Answer:
(a) On your calculator, take the log of 1.4...

Calculating pOH The [OH^-] of a strongly basic solution is 1.0 * 10^-2. What are the pOH and pH of this solution? Strategy When given the [OH^-], determine the pOH by taking the negative logarithm. To calculate the pH, subtract the pOH from 14.

Verified Answer:
The pOH is -log 1.0 \times 10^{-2} ...

Titrations Following are data for the titration of 0.108 M H2SO4 with a solution of NaOH of unknown concentration. What is the concentration of the NaOH solution? Strategy Use the volume of the acid and its concentration to calculate how many moles of hydrogen ions are available to be titrated. At

Verified Answer:
From the balanced equation for this acid–base reac...

Buffers What is the pH of a buffer solution containing equimolar quantities of (a) H3PO4 and NaH2PO4? (b) H2CO3 and NaHCO3? Strategy When there are equimolar quantities of a weak acid and its conjugate base in a buffer solution, the pH is always the same as the pKa of the weak acid. Look up the pKa

Verified Answer:
Because we are adding equimolar quantities of a we...

Buffer pH Calculation What is the pH of a phosphate buffer solution containing 1.0 mol/L of sodium dihydrogen phosphate, NaH2PO4, and 0.50 mol/L of sodium hydrogen phosphate, Na2HPO4? Strategy Use the Henderson-Hasselbalch equation to determine the pH. You must know either the number of moles of

Verified Answer:
Solution The weak acid in this problem is H...

pKas . Ka for benzoic acid is 6.5 x 10^5. What is the pKa of this acid?Strategy :The pKa is -log Ka. Thus, use your calculator to find the log of the Ka and then take the negative of it.

Verified Answer:
Take the logarithm of 6.5  \times  10^{-5}[...

Diprotic Acids . Show how the amphiprotic ion hydrogen sulfate, HSO4^-, can react as both an acid and a base.Strategy : For a molecule to act as both an acid and a base, it must be able to both give up a hydrogen ion and accept a hydrogen ion. Therefore we write two equations, one donating a

Verified Answer:
Hydrogen sulfate reacts as an acid in the equation...