Answer:
Chromium
Explanation:
Cr has 24 atomic number and mass number 52
Explanation:
An acid is a substance that produces excess hydroxonium ions in solution.
An acid based on the pH scale is a substance that has a low pH. Acid lies within a range of 1-7 on the pH scale.
- A pH of 7 is for neutral compounds like water.
- A pH greater that 7 is for basic compounds.
- In order to raise the pH, we are driving at a substance becoming more neutral or basic.
This can be achieved by adding more base to the solution of the substance. When we add more base, hydroxyl ions will neutralize the excess hydroxonium ions and drag the pH towards that of neutrality.
Addition of more base can eventually make the substance basic.
learn more:
Phosphoric acid brainly.com/question/11062486
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The individual can consume less than 184.6 g of the snack mix and still be within the FDA limit of salt consumption.
<h3>What is the mass of snack that can be consumed within the limit of sodium intake?</h3>
The mass of the snack mix that the individual can consume and still be within the FDA limit is calculated as follows:
U.S. Food and Drug Administration (FDA) recommends of sodium intake = less than 2.40 g of sodium per day.
Amount of salt in 100 g of snack mix = 1.30 g
Mass of snack that will contain 2.40 g of sodium = 2.40 * 100g/1.30 = 184.6 g of snack mix
Therefore, the individual can consume less than 184.6 of the snack mix and still be within the FDA limit of salt consumption.
In conclusion, the FDA recommends that an individual take in less than 2.40 g of sodium per day from their diet.
Learn more about salts at: brainly.com/question/23463868
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Answer:
Attached is the solution to the question
Explanation:
Answer:
![\large \boxed{\text{0.180 mol/kg }}](https://tex.z-dn.net/?f=%5Clarge%20%5Cboxed%7B%5Ctext%7B0.180%20mol%2Fkg%20%7D%7D)
Explanation:
Assume 100 g of solution.
Then you have 10.0 g of NaCl and 90.0 g of water.
![\text{Molal concentration} = \dfrac{\text{moles of solute}}{\text{kilograms of solvent}}](https://tex.z-dn.net/?f=%5Ctext%7BMolal%20concentration%7D%20%3D%20%5Cdfrac%7B%5Ctext%7Bmoles%20of%20solute%7D%7D%7B%5Ctext%7Bkilograms%20of%20solvent%7D%7D)
1. Moles of NaCl
![\text{Moles of NaCl} = \text{10.0 g NaCl} \times \dfrac{\text{1 mol NaCl}}{\text{58.44 g NaCl}} = \text{0.1711 mol NaCl}](https://tex.z-dn.net/?f=%5Ctext%7BMoles%20of%20NaCl%7D%20%3D%20%5Ctext%7B10.0%20g%20NaCl%7D%20%5Ctimes%20%5Cdfrac%7B%5Ctext%7B1%20mol%20NaCl%7D%7D%7B%5Ctext%7B58.44%20g%20NaCl%7D%7D%20%3D%20%5Ctext%7B0.1711%20mol%20NaCl%7D)
2. Kilograms of water
![\text{Kilograms} = \text{90.0 g} \times \dfrac{\text{1 kg}}{\text{1000 g}} = \text{0.0900 kg}](https://tex.z-dn.net/?f=%5Ctext%7BKilograms%7D%20%3D%20%5Ctext%7B90.0%20g%7D%20%5Ctimes%20%5Cdfrac%7B%5Ctext%7B1%20kg%7D%7D%7B%5Ctext%7B1000%20g%7D%7D%20%3D%20%5Ctext%7B0.0900%20kg%7D)
3. Molal concentration
![\text{Molal concentration} = \dfrac{\text{0.1711 mol}} {\text{0.0900 kg}} = \textbf{1.90 mol/kg}\\\\\text{The molal concentration of the solution is $\large \boxed{\textbf{0.180 mol/kg }}$}](https://tex.z-dn.net/?f=%5Ctext%7BMolal%20concentration%7D%20%3D%20%5Cdfrac%7B%5Ctext%7B0.1711%20mol%7D%7D%20%7B%5Ctext%7B0.0900%20kg%7D%7D%20%3D%20%5Ctextbf%7B1.90%20mol%2Fkg%7D%5C%5C%5C%5C%5Ctext%7BThe%20molal%20concentration%20of%20the%20solution%20is%20%24%5Clarge%20%5Cboxed%7B%5Ctextbf%7B0.180%20mol%2Fkg%20%7D%7D%24%7D)