## How much water would I need to add to 500 mL of a 2.4 M KCl?

5) How much water would I need to add to 500 mL of a 2.4 M KCl solution to make a 1.0 M solution? **1200 mL** will be the final volume of the solution. However since there’s already 500 mL of solution present you only need to add 700 mL of water to get 1200 mL as your final volume. The answer: 700 mL.

## How do you calculate molarity of KCl?

One mol of KCl is equal to **74.6 grams** (from the periodic chart the gram-atomic mass of potassium is 39.0 and that of chlorine is 35.5. Add together for the gram-molecular mass of 74.6). If you took 74.6 grams of KCl and diluted this to one liter with water you would have a 1.00 M KCl solution.

## How much KCl in grams should the chemist use?

Molarity(M) is defined as number of moles of solute dissolved in one litre (or one cubic decimetre) of solution. = **18.64 g**. Thus the required mass of KCl is 18.64 g.

## How do you calculate 3M KCl solution?

**To make 125 mL of 3M KCl**

- Using digital scale place 27.96 g KCl powder into weigh boat.
- In 150 mL flask mix 27.96 g KCl with 100 mL H
_{2}O. - Put flask on hotplate/stirrer with stirbar until dissolved.
- Add H
_{2}O to bring volume to 125 mL.

## How much water would need to be added to 500 mL of a 2.4 M KCl solution to make a 1.0 M solution?

**1200 – 500 = 700 mL**.

## How many grams of potassium carbonate are needed to make 2.00 102 mL 200 mL of a 2.5 M solution?

**70 g** of potassium carbonate.

## How many grams of KCl would be dissolved in 60g?

**15 g** is the required answer.

## How many grams of KNO3 are needed to make 250 mL of a solution that is .135 M?

– So the amount of potassium nitrate (KNO3) required to make the solution is **10.1 gm**.

## What volume of 12.0 M HCl is required to?

**21.9 mL** of a 12.0 M HCl solution is needed to make 75 mL of a 3.5 M solution.

## What is the molar mass of KCl?

Potassium chloride/Molar mass

Answer and Explanation: The molar mass of a compound is calculated by multiplying the sum of the relative atomic mass Ar of the constituent atoms by the molar mass constant Mu . Where Mr is the relative molar mass. Hence the molar mass of KCl is obtained as 74.5513 g mol−1 74.5513 g m o l − 1 .

## What is 3M KCl solution?

Potassium Chloride Electrolyte Standard Solution 3M Chem-Lab is a filling solution for pH electrodes **containing 224g KCl per liter of water**. … It is used for proper electrode storage to maintain optimal electrode performance.

## How do you make KCl solution?

For a 1 M solution of KCl **dissolve 74.55 g of KCl in** 900 mL of H_{2}O. Make up the volume to 1 L with H_{2}O and autoclave for 20 min on liquid cycle.

## How do you make a KCl solution saturated?

**In our bottles there are always crystals of KCl in excess to ensure saturation.**

- KCl solubility at 20°C: 0 340 g·cm-3 in water = 340 g/l = 4.56 mol/l (Saturated KCl at 20°C)
- KCl solubility at 30°C: 0 374 g·cm-3 in water = 374 g/l = 5.02 mol/l (Saturated KCl at 30°C)

## What volume of water should be added to 2.6 g of KCl to make a 4 M solution?

**8.7ml**Acid/Base: The Water Constant and pH Instructions: Determine if each solution is acidic basic or neutral.

## What is molarity of a solution in which 63 gm nitric acid is dissolved in 1 Litre solution?

**1.2 M**. 63% weight means 63 gm of $HN{O_3}$ is present in 100 g of solution.

## How many mL of 10.0 m NaOH do you need to add to 100 mL of 1.00 M NaOH to get a solution that is 5.00 m?

How many ml of 10.0 M NaOH do I need to add to 100 ml of 1.00 M NaOH to get a solution that is 5.00 in NaOH? Let x ml of 10.0 M NaOH have to added with the 100 ml of 1.00 M NaOH solution. Hence **60 ml** of 10.0 M NaOH need to add to get the solution of required strength.

## How many grams of ammonium sulfate are needed to make a 0.25 M solution at a concentration of 6 m?

0.25 L of a solution with a molarity of 6M has 6*0.25 = 1.5 moles of the solute. The molar mass of ammonium sulfate is 132.14 g/mole. The mass of 1.5 moles is 132.14*1.5 = 198.21 g. Therefore **198.12 g** of ammonium sulfate are required to make 0.25 L of a solution with a concentration of 6M.

## How many grams of potassium carbonate are needed to make 200 ml of a 2.5 M solution hint use molarity formula but you are solving for solute not molarity?

Hence **69 grams** of potassium carbonate $ {K_2}C{O_3} $ are needed to make $ 200{text{ }}mL $ of a $ 2.5{text{ }}M $ solution.

## How do you make 2M K2CO3?

(iii) 2M K2CO3 (Potassium Carbonate): Dissolve 276.41 g K2CO3 in 1000 ml **distilled water**. (iv) 0.25M Na2CO3 (Sodium Carbonate): Dissolve 26.5 g Na2CO3 in 1000 ml distilled water. (v) 1M CH3COOH (Acetic Acid 99.5% assay ρ = 1.05g/cm3): Dissolve 57.192 ml CH3COOH and make up the volume to 1000 ml with distilled water.

## How many grams of KCl must be added?

Answer: **12.6 grams** of KCl must be added to 75.0g of water to produce a solution that is 2.25 molal. Explanation: Molality is defined as the moles of solute dissolved per kg of the solvent.

## How many grams of KCl should be added?

– So 1 ml of 1 M KCl contains about 74.5 / 1000 grams of KCl. – Now 500 ml of 1 M KCl contains about (74.5 / 1000) X 500 gm of KCl. – Hence we can conclude that the correct answer is option (c) that is **37.3 g grams** of potassium chloride (KCl) must be added to make 500 ml of M KCl solution.

## How many grams of salt should be dissolved in 60 gram of water so as to prepare 25% weight by weight solution?

∴A = **10.6** ( approx. )

## How many grams of AgNO3 are needed to make 250 mL of a solution that is 0.140 M?

Answer and Explanation: The mass of AgNO3 A g N O 3 needed is **5.95 g**.

## How much KNO3 in grams is needed?

## How many milliliters are in a 9.0 m h2so4 solution?

**175 milliliters** (mL) of a 9.0 M H_{2}SO_{4} solution is needed to make 0.45 L of a 3.5 M solution.

## What volume of 12.0 M HCl a common laboratory stock solution must be used to prepare 250.0 mL of 0.125 M HCl?

Question: What volume of 12.0 M HCl a common laboratory stock solution must be used to prepare 250.0 mL of 0.125 M HCl? The answer I got: **2.60 mL**.

## What volume of HCl must be diluted to 250ml water to obtain 0.6 M solution from stock solution of 12M?

**62.5 mL** of HCl is required.

## How do you dilute 12M HCl to 3 M HCl?

So we need **12.5 mL of** the 12 M HCl diluted with water up to 50 mL to create a 3 Molar HCl solution.

## How do you calculate the formula mass of KCl?

Potassium chloride/Molar mass

Multiply the number of atoms for each chemical multiplied by the atomic mass. Add up the results from multiplying the numbers to obtain the molar mass for the compound. For example for KCl (1 atom X 39.0983 Potassium) + (1 atom X 35.453 Chlorine) = (74.5513 g/mol) which is the molar mass for KCl.Apr 24 2017

## What is the mass ratio of KCl?

This means that every sample of potassium chloride regardless of its mass will contain **47.55%** chlorine and 52.45% potassium. So as a conclusion any two samples of potassium chloride will contain potassium and chlorine in a 0.9068 : 1 or 52.55% to 47.55% mass ratio.

## How many moles are in 25.0 grams of KCl?

**25122.4** = moles.

## How do you store pH probes?

Always keep your pH electrode moist. We recommend that you store your electrode in **a solution of 4 M KCl**. If 4 M KCl is not available use a pH 4 or 7 buffer solution. DO NOT store electrode in distilled or deionized water—this will cause ions to leach out of the glass bulb and render your electrode useless.

## What is the normality of KCl?

**One mol of KCl is equal to 74.6 grams**(from the periodic chart the gram-atomic mass of potassium is 39.0 and that of chlorine is 35.5.

…

Lagoon. Systems In Maine.

Acidity and Alkalinity | Normality |
---|---|

Method Detection Limits | Total Suspended Solids |

Molarity | |

pH Measurements | |

Nitrogen |

## What is the pH of 0.1 M KCl solution?

pH of KCl aqueous solution is **7** because in KCl both cation and anion are spectator ion which are not hydrolysed .

## How many grams of KCl are needed to prepare 500 mL of a 1.20 M KCl stock solution?

## Molarity Dilution Problems Solution Stoichiometry Grams Moles Liters Volume Calculations Chemistry

## How to Calculate Mass Needed to Make a Solution

## How many mL of a 0.345M phosphoric acid solution are required to neutralize 125 mL of a 0.123M KOH solution?