What is the final concentration of the solution produced when 225.5 mL of 0.09988 M solution of...
Question:
What is the final concentration of the solution produced when 225.5 mL of 0.09988 M solution of {eq}Na_2CO_3 {/eq} is allowed to evaporate until the solution volume is reduced to 45.00 mL?
Molarity:
The amount of solute dissolved in a solution defines the concentration of the solution. An expression of a solution's concentration is molarity, M, which can be calculated using the formula below:
{eq}\rm M = \dfrac{n}{V} {/eq}
where {eq}\rm n{/eq} is the moles of the solute and {eq}\rm V{/eq} is the volume of the solution.
Answer and Explanation: 1
We first calculate for the number of moles, n, of sodium carbonate, {eq}\rm Na_2CO_3 {/eq}, present in the given volume V of the solution, 225.5 mL or 0.2255 L, whose concentration M is 0.0988 M. Using the formula below, the moles of sodium carbonate is:
{eq}\rm n = MV = 0.09988 \frac{mol~Na_2CO_3}{L} (0.2255~L) = 0.0225229~mol~Na_2CO_3 {/eq}
This mole is also the same number of moles of sodium carbonate when the volume of the solution was reduced to 45.00 mL or 0.04500 L. We can calculate for the new molarity of the solution as follows:
{eq}\rm M = \dfrac{moles~Na_2CO_3}{volume~solution} = \dfrac{0.0225229~mol~Na_2CO_3}{0.04500~L} = \boxed{\mathbf{0.5005~M}} {/eq}
Ask a question
Our experts can answer your tough homework and study questions.
Ask a question Ask a questionSearch Answers
Learn more about this topic:

from
Chapter 8 / Lesson 4What is molarity? What is molality? Compare molarity vs molality by viewing molality and molarity formulas, how to calculate molarity and molality, and examples.
Related to this Question
- What is the final concentration of the solution produced when 275.0 mL of a 0.098 M solution of Na2CO3 is allowed to evaporate until the solution volume is reduced to 75.0 mL?
- What is the final concentration of the solution produced when 225.5 ml of a 0.09988 M solution of Na_2CO_3 is allowed to evaporate until the solution volume is reduced to 45.00 ml?
- What is the molarity of 5.30 g of Na2CO3 dissolved in 400.0 mL solution?
- What is the molarity of 5.65 g of Na2CO3 dissolved in 450 mL of solution?
- What is the molarity of 8.20 g of Na2CO3 dissolved in 350.0 mL of solution?
- What is the molarity of a solution that contains 8.25 g of Na2CO3 in 450 mL of solution?
- What is the molarity of a solution made when you dilute 35 grams of sodium carbonate (Na_2CO_3) to a volume of 3,400 mL?
- If 25.00 mL of 1.04 M Na_2CO_3 is diluted to 0.500 L, what is the molarity of Na_2CO_3 in the diluted solution?
- What volume (in mL) of 1.50 M Na2CO3 solution can be prepared from 3.975 g of solid Na2CO3?
- Suppose 17.5 mL of a 0.1050 M Na2CO3 solution is added to 46.0 mL of a 0.1250 M NaCl solution. What is the concentration of sodium ions in the final solution?
- What is the OH- concentration of a 0.16 M in Na2CO3 solution?
- What is the OH- concentration of a solution that is 0.28 M in Na2CO3?
- What is the molarity of a solution prepared by dissolving 10.60 g of Na_2CO_3 in enough distilled water to obtain 250.0 ml of solution?
- How many grams of Na_2CO_3 are present in 29.5 ml of a solution that is 31.0 % Na_2CO_3 by mass? The density of the solution is 1.15 g/ml.
- 20 ml of a solution of HCl concentration, neutralized 0.50 g of Na_2CO_3. What is the Molarity of the acid solution?
- Assume that 4.16 grams of Na_2CO_3 is dissolved in 200 mL water. \\ 1. What is the molarity of Na_2CO_3 in the solution? 2. What is the molarity of each ion in the solution?
- Choose the answer which gives the concentration of each ion present in the solution formed by mixing together the two solutions described below: 40.6 mL of 0.267 M Na_2CO_3 and 15.5 mL of 0.531 M Na_
- What is the concentration of Na^+ in a 0.73 M Na2CO3 solution?
- What is the concentration of the NaCl solution that results when 0.150 L of a 0.60 M solution is allowed to evaporate until the volume is reduced to 0.075 L?
- How many grams of Na_2CO_3 are present in 18.4 mL of a 34.0% Na_2CO_3 solution? The density of the solution is 1.10 g/mL.
- A solution is prepared by dissolving 49.73 g of Na_2CO_3 in water to a total volume of 800.0 mL. Then, 5.00 mL of this solution was diluted with water to a total volume of 40.0 mL. What are the concentrations of each of the ions in the diluted solution?
- A 5.317 g sample of Na2CO3 is dissolved in enough water to make 170.0 mL of solution. a) What is the molarity of the solution? b) How much additional water must be added to this solution in order for its concentration to be reduced to 0.125 M? c) What
- A 5.317 g sample of Na2CO3 is dissolved in enough water to make 170.0 mL of solution. a) What is the molarity of the solution? b) How much additional water must be added to this solution in order for its concentration to be reduced to 0.125 M? c) What mas
- How many grams of Na2CO3 are present in 29.3 mL of a 22.0% by mass Na2CO3 solution? The density of the solution is 1.09 g/mL.
- What is the molarity of a solution made when you dilute 35 grams of sodium carbonate (Na2CO3) to a volume of 3,400 mL?
- What is the final concentration (M) of a solution prepared by diluting 50.0 mL of a 6.00 M KCl solution to a volume of 0.500 L? A) 0.0167 B) 1.67 C) 3.0 D) 0.600
- How many moles of Na2CO3 are in 10.0 mL of a 2.0 M solution?
- A solution of sodium carbonate contains 1.06 g of Na2CO3 dissolved in 100 mL of water. Calculate its concentration in normality. (d = 2.54 g/mL)
- What volume of a 0.921 M Na2CO3 solution contains 74.0 grams of Na2CO3?
- What volume of 0.745 M Na2CO3 (106 g/mol) solution contains 50.3 grams of Na2CO3?
- Suppose you dissolve 52.2 g of Na_2CO_3 - xH_2O in enough water to make 5.00 L of solution. The final concentration of the solution was found to be 0.0366 M. D...
- 1.00 g Na_{2}CO_{3} is dissolved in 50.00 mL H_{2}O and titrated with HCl. 18.0 mL of a HCl solution were required to titrate the Na_{2}CO_{3} solution. What is molarity of HCl solution? Na_{2}CO_{3}(aq)+2HCl(aq)\rightarrow2NaCl(aq)+H_{2}O(l)+CO_{2}(g)
- What volume of 10 percentage (mass/volume) solution of Na2CO3 will be required to neutralize 100 mL of HCl solution containing 3.65 g of HCl?
- If 100 ml of a 1.0 m solution is evaporated to a volume of 25ml, what will be the concentration of the resulting solution ? 1) 0.25 M 2) 0.50 M 3) 2.0 M 4) 4.0 M
- What is the final concentration (M) of a solution prepared by diluting 50.0 mL of a 6.00 M KCl solution to a volume of 0.500 L? A. 1.67. B. 0.600. C. 0.0167. D. 3.0. E. None of these.
- What volume of 0.18M Na_2CO_3 would neutralize 25ml of the HCL solution?
- What is the concentration of a solution made by diluting 75 mL of 6.0 M HCl to a final volume of 750 mL?
- What is the concentration of a solution made by diluting 55 ml of 6.0 M HCl to a final volume of 750 ml?
- What is the concentration of a solution made by diluting 25 mL of 6.0 M HCl to a final volume of 750 mL?
- What is the concentration of a solution made by diluting 35 ml of 6.0 M HCL to a final volume of 750 ml?
- What is the concentration of a solution made by diluting 95 mL of 6.0 M HCl to a final volume of 750 mL?
- What is the concentration of a solution made by diluting 85 mL of 6.0 M HCI to a final volume of 750 mL?
- What is the concentration of a solution made by diluting 15 mL of 6.0 M HCI to a final volume of 750 mL?
- What is the concentration of a solution made by diluting 35 mL of 6.0 M HCI to a final volume of 750 mL? ................ M
- What is the concentration of a solution made by diluting 45 mL of 6.0 M HCl to a final volume of 750 mL?
- What is the concentration of a solution made by diluting 65 mL of 6.0 M HCl to a final volume of 750 mL?
- If 106 g of Na_2CO_3 is dissolved in 6.00 L H_2O , what is the molarity of this solution?
- Molarity Sodium carbonate (Na_2CO_3) is available in very pure form and can be used to standardize acid solutions. What is the molarity of an HCI solution if 23.3 mL of the solution is required to rea
- 1) In the laboratory, you dissolve 23.1 g of sodium carbonate in a volumetric flask and add water to a total volume of 500 mL. a) What is the molarity of the solution? b) What is the concentration o
- A solution was prepared by dissolving 4.55 grams of Na_2CO_3 in 75.0 grams of water. What is the % Na_2CO_3 (by mass) in the resulting solution? a) 6.46 % b) 6.07 % c) 94.3 % d) 5.72 %
- How many grams of Na_2CO_3 are required to prepare a 125 mL of 3.12 M solution?
- What is the concentration of a solution of lithium carbonate containing 0.01 mol in 750 mL of the solution?
- Calculate the concentration of these solutions: a. 2.86 g sodium carbonate crystals, Na2CO3 b. 10H2O dissolved in 250 cm^3 of solution
- A solution of HCl is approximately 0.1 M and has to be standardized. 1.234 g Na2CO3 is dissolved to make 100 mL of solution. 20 mL of this solution is titrated with the HCl solution, requiring 31.3 mL
- A 331 mL sample of unknown HCl solution reacts completely with Na2CO3 to form 19.1 g of CO2. What was the concentration of the HCl solution?
- A 557-mL sample of unknown HCl solution reacts completely with Na2CO3 to form 19.1 g of CO2. What was the concentration of the HCl solution?
- A 427-mL sample of an unknown HCl solution reacts completely with Na2CO3 to form 14.1 g of CO2. What was the concentration of the HCl solution?
- A 337-mL sample of unknown HCl solution reacts completely with Na2CO3 to form 17.1g CO2. What was the concentration of the HCl solution?
- A 331 mL sample of unknown HCl solution reacts completely with Na2CO3 to form 13.1 g CO2. What was the concentration of the HCl solution?
- A 495 mL sample of unknown HCl solution reacts completely with Na_2CO_3 to form 18.1 g CO_2. What was the concentration of the HCl solution?
- Strong acid solutions may have their concentration determined by reaction with measured quantities of standard sodium carbonate solution. What mass of Na2CO3 is needed to prepare 250. mL of 0.0500 M Na2CO3 solution?
- a. If 6.73 g of Na_2CO_3 is dissolved in enough water to make 250.0 mL of solution, what is the molar concentration of the sodium carbonate? b. What are the molar concentrations of the Na^+ and CO_3^{2-} ions?
- You mix 25.2 mL of a 1.07 M NiCl_2 solution with 61.6 mL of a 0.338 M Na_2CO_3 solution, leading to the precipitation of NiCO_3. Calculate the concentration of the chloride ion in the resulting solution.
- 3. What volume of a 0.500M HCl solution is needed to neutralize 10.0 mL of a 0.200 M Ba(OH)_2 solution. 4. 17.5 mL of a 0.1050 M Na_2CO_3 solution is added to 46.0 mL of 0.1250 M NaCl. What is the co
- If 21.9 mL of an HCl solution is required to neutralize 1.152 g of Na2CO3, what is the molarity of the HCl solution?
- What is the concentration of aqueous KCI solution that results when 0.15 L of a 0.556 M solution is allowed to evaporate until the volume is reduced to 0.105 L?
- What is the molarity of a solution made by dissolving 10.0 grams of NaHCO3 in water where the final volume is 2 liters?
- What is the final volume. In milliliters, when 10 0 mL of each of the following solutions is diluted to provide the given concentration? 11.5%(m/v) HC1 solution to give a 3 50 %(m/v) HC1 solution 4.00
- A 501-mL sample of unknown HCl solution reacts completely with Na2CO3 to form 12.1 grams of CO2. What was the concentration of the HCl solution?
- A 327 ML sample of unknown HCI solution reacts completely with Na_2CO_3 to form 20.1 g CO_2. What was the concentration of the HCI solution?
- What is the concentration of the solution which is formed when 0.4 moles of HCl is dissolved to form 75 mL of solution? a. 5.3 mol/L b. 1.0 mol/L c. 2.0 mol/L d. 13.3 mol/L
- 30 mL of 0.10 M Ba(NO_3)_2 is added to 10 mL of 0.10 M Na_2CO_3 and resulting concentration in solution of Ba is 0.075 M CO_3 is 0.025 M. What is the value of the reaction quotient?
- If you take an 11.5 mL sample of a 12.6 M NH3 solution and dilute it to a total volume of 0.650 L, what will be the concentration of the final solution?
- Calculate the molarity of sodium carbonate in a solution prepared by dissolving 5.9 g in enough water to form 250 ml of solution.
- What is the molarity of a 12.6% solution of sodium carbonate with a density of 1.31 g/mL?
- What is the concentration of the solution prepared by diluting 0.200 L of a 2.00 M solution to a final volume of 0.800 L? a) 8.00 M b) 0.200 M c) 0.500 M d) 0.400 M e) 0.800 M
- What is the concentration of the solution which is formed when 1.0 mole of HCL is dissolved to form 75 mL of solution?
- What is the concentration of a solution that is made by diluting 225 mL of a 12.3% (w/v) solution to 750 mL?
- If 120 mL of a 6 M N a O H solution is diluted to a final volume of 200 mL, what is the resulting concentration of the solution?
- 1.06 g of Na2CO3 is dissolved in water to make a 250 cm^3 solution. 10.0 cm^3 of this solution was further diluted to make 500 cm^3 of a second solution. 25.0 cm^3 of the second solution reacted with
- Calculate the molarity of sodium carbonate in a solution prepared by dissolving 5.3 gram in enough water to form 250 ml of solution.
- Calculate the volume of a 2.0 M solution of sodium carbonate required to make 100 mL of a 0.25 M solution.
- 25 mL of a solution of Na2CO3 having a specific gravity of 1.25 g mL required 32.9 mL of a solution of HCl containing 109.5 g of the acid per liter for complete neutralization. Calculate the volume of
- What is the concentration of a solution created by diluting 5.0 mL of a 0.90 M solution to 80.0 mL?
- What mass of sodium carbonate must be used to get a 300.0 mL solution with a 2.50 mol/L concentration? And what volume of water must 60.0 g of potassium hydroxide be added to in order to get a 0.10 mol/L solution?
- Determine the mass (in grams) of NiCO3 that is produced when 93.7 mL of a 1.86 x 10-2 M Na2CO3 solution completely reacts with 564 mL of an 8.14 x 10-2 M NiCl2 solution.
- Find the molarity of a HCl solution if 25.5 mL of HCl is required to neutralize 0.375g of Na2CO3 as shown in the following equation: 2HCl(aq) + Na2CO3(aq) -> 2 NaCl(aq) + H2O(l) + CO2(l)
- A 565-mL sample of unknown HCl solution reacts completely with Na_2CO_3 to form 14.1 grams of CO_2. What was the concentration of the HCl solution? 2HCl(aq) + Na_2CO_3(aq) ---> 2NaCl(aq) + H_2O(l) + CO_2(g)
- Explain how you could prepare 100 mL of a 0.25 M Na2CO3 solution from a 4.0 M Na2CO3 solution.
- Calculate the molarity of an HCl solution if 39.1 mL of the solution reacts with 0.483 g of Na2CO3.
- What is the concentration of Na and CO_3 ions in 0.2M aqueous solution of Na_2CO_3?
- Assume that 6.73 g of Na2CO3 is dissolved in enough water to make 250 mL of solution. a. What is the molarity of the sodium carbonate? b. What are the concentrations of the Na+ and CO32- ions?
- Your standardized NaOH(aq) solution is 0.202 M: Your standardized HCl(aq) solution is 0.175 M. Some mass of Na_2CO_3 has been added to 25.00 ml of your 0.175 M HCl(aq) solution. After warming to remove the CO_2(g) you find that 11.30 ml of your 0.202 M Na
- What is the molarity of a KMnO_{4} solution if the endpoint was reached after pouring 20.55 mL of KMnO_{4} into 20.00 mL of H_{2}C_{2}0_{4} solution (concentration = 0.0505 M)? a. 0.0197 M b. 20.3 M c. 0.123 M d. 0.0491 M e. 0.0584 M
- Determine the concentrations of Na_2CO_3, Na , and CO_3^{2-} in a solution prepared by dissolving 2.22 \times 10^4 g Na_2CO_3 in 2.25 L of water. Express all three concentrations in molarity. Additionally, express the concentrations of the ionic species
- The density of 8.653 % Na_2CO_3 solution is 1.018 g / ml. What is the molality of the solution?
- When 50.0 mL of 0.2 M Na2CO3 is combined with 30.0 mL of 0.50 M NaCl, what is the concentration of ions?
- What is the concentration of the solution prepared by diluting 0.200 L of a 2.00 M solution to a final volume of 0.800 L?
- What is the final volume (in Litres) of a solution prepared by diluting 25 mL of 8.25 M sodium hydroxide to a concentration of 2.40 M?
- The procedure for an experiment calls for 100 mL of 0.300 M Na_2CO_3 solution. However, the stock room only stores solutions of 10.0 M Na_2CO_3. What volume of 10.0 M Na_2CO_3 and dilute to produce the 100 mL of 0.300 M Na_2CO_3?