The** volume **of 0.160 M **sulfuric acid **necessary to react completely with 75.0 g **sodium hydroxide** **is 0.15L**

The** reaction** of** sulphuric acid** and sodium hydroxide is expressed as:

Determine the **moles of NaOH** present

Molar mass of NaOH = 23 + 16 + 1 = 40g/mole

Given that mass of NaOH is 75.0g

**Mole of NaOH** = 75/40 = 1.875moles

Determine the **number of moles ** needed to **react **with **1.875 moles NaOH**

Moles of =

Recall that volume = Molar mass * number of moles

Volume of = 0.160 * 0.9375

Volume of = 0.15L

Hence the** volume **of 0.160 M **sulfuric acid **necessary to react completely with 75.0 g **sodium hydroxide** **is 0.15L**

**Learn more here: brainly.com/question/837939**

**
**

STP means standard temperature and pressure which is equivalent to 273 K and 1 atm, respectively. Assuming ideal gas behavior, the solution for this problem is as follows:

PV = nRT

Solve for n,

n = RT/PV

n = (0.0821 L-atm/mol-K)(273 K)/(1 atm)(1×10⁵ L)

**<em>n = 2.24×10⁻⁴ moles</em>**

**Answer:**

The property of ever heterogeneous mixture is a solid dissolved into a liquid.

**Explanation:**