A 327 ML sample of unknown HCI solution reacts completely with Na_2CO_3 to form 20.1 g CO_2. What...
Question:
A {eq}327 \ ML {/eq} sample of unknown {eq}HCI {/eq} solution reacts completely with {eq}Na_2CO_3 {/eq} to form {eq}20.1 \ g \ CO_2 {/eq}. What was the concentration of the {eq}HCI {/eq} solution?
Carbonic Acids:
When a carbonate is neutralized with excess acid, carbonic acid forms. However, the solution will effervesce, forming carbon dioxide and water from the decomposition of the carbonic acid.
{eq}\displaystyle 2HCl + CO_3^{2-} \rightarrow 2Cl^- + H_2O + CO_2 {/eq}
Answer and Explanation: 1
Become a Study.com member to unlock this answer! Create your account
View this answerMolar mass of carbon dioxide = 44.01 g/mol
By stoichiometry, the moles of HCl in the solution is:
{eq}\displaystyle 20.1 \ g \times \frac{1 \ mol \...
See full answer below.
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:
Get access to this video and our entire Q&A library
Calculating Molarity and Molality Concentration
from
Chapter 8 / Lesson 4
67K
What 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
- 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 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 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 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 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?
- 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 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)
- A 651-mL sample of unknown HCl solution reacts completely with Na2CO3 to form 12.1 g of CO2. What was the concentration of the HCl solution? 2HCl(aq) + Na2CO3(aq) arrow 2NaCl(aq) + H2O(l) + CO2(g)
- A 559-mL sample of unknown HCl solution reacts completely with Na2CO3 to form 18.1 g CO2. What was the concentration of the HCl solution? Express your answer to three significant figures and include the appropriate units.
- 20 ml of a solution of HCl concentration, neutralized 0.50 g of Na_2CO_3. What is the Molarity of the acid solution?
- If it takes 10.25 mL of HCI titrant to reach the endpoint for a sample containing 0.125 g of Na2CO3, what is the molarity of the HCI solution?
- A 331-mL sample of unknown HCl solution reacts completely with Na_2CO_3 to form 16.1 g CO_2. What was the concentration of the HCl solution? Express your answer to three significant figures and include the appropriate units.
- 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?
- 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)
- 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
- Calculate the molarity of an HCl solution if 39.1 mL of the solution reacts with 0.483 g of Na2CO3.
- A 30 mL sample of an unknown concentration was titrated with 35.5 mL of .083 M NaOH. What is the concentration of the HCI?
- We can measure the concentration of HCl solution by reaction with pure sodium carbonate. A volume of 20.35 \pm 0.03 mL of HCl solution was required for complete reaction (reach both endpoints) with 0.9674 \pm 0.0009 g of Na_2CO_3 (FM 105.988). Find the ml
- You have a sample of HCl with an unknown concentration. Suppose 10.00 mL of this solution is titrated with 12.54 mL of 0.100 M NaOH. What is the unknown HCl concentration?
- 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
- What is the molarity of an HCI solution if 30.3 mL of that solution is required to react with 0.185 g of Na2CO3? 2HCl + Na2CO3 arrow 2NaCl + H2O + CO2
- If 40.37 ml of an HCl solution were required to titrate a solution containing 221.4 mg of primary standard sodium carbonate, and calculate the molar concentration of the HCl 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)
- What is the concentration of HCl if 21.5 mL of HCl was needed to react with 0.611 g of Na_2CO_3 to reach the endpoint?
- A 35.0 mL sample of an NH3 solution is titrated with a 0.25 M HCl solution. At the endpoint, it is found that 45.0 mL of HCl was used. What was the concentration of the NH3 solution?
- What volume of 0.18M Na_2CO_3 would neutralize 25ml of the HCL solution?
- The titration of 25.0 mL of an HCl solution of unknown concentration requires 14.8 mL of 0.100 M NaOH. What is the molar concentration of the HCl solution?
- Concentrated HCI is 12 M. What is the molarity of an HCI solution prepared by dilluting 10 ml concentrated HCI to a total volume of 250 ml?
- A student found that 0.4131 g Na_2CO_3 was required to reach the equivalence point when added to 25.00 mL of a solution of HCl of unknown concentration. What is the concentration of the acid solution?
- A 24.9-mL volume of hydrochloric acid reacts completely with 55.0 mL of aqueous Na2CO3. The volume of CO2 formed is 141 mL at 27 C and 727 mmHg. What is the molarity of the HCl solution?
- When performing a titration, 23.65 mL of 1.25 M calcium carbonate was used to neutralize 9.68 mL of HCl. What is the concentration of the HCl solution?
- You have 45.0 mL HCI of unknown concentration. It takes 22.5 mL of 0.2 M NaOH to neutralize the acid. Determine the concentration of HCI.
- 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?
- The concentration of HCl can be determined by titration with a primary standard such as Na_2CO_3 (sodium carbonate). The titration reaction is: CO_3^{2-} + 2H^+ to H_2O + CO_2. What is the concentration of HCl if 35.7 mL of HCl was needed to to react with
- Suppose that it takes 25.0 mL of a 0.100 M NaOH solution to titrate 20.00 mL of an HCl solution of unknown concentration. What is the molarity of the unknown HCl solution?
- If it takes 54 mL of 0.1 M NaOH to neutralize 125 mL of an HCI solution, what is the concentration of the HCI?
- Concentrated HCI is 12 M. What is the molarity of an HCI solution prepared by diluting 10 ml concentrated HCI to a total volume of 250 ml?
- A 25.0-mL sample of HCl solution of unknown concentration is titrated with a 0.150 M NaOH solution. If 38.6 mL of the NaOH solution is required to neutralize the acid solution, what is the concentration of the HCl solution?
- Concentrated HCI is 12 M. What is the molarity of an HCI solution prepared by diluting 10 mL of concentrated HCI.
- If it takes 5 mL of 1.4 M NaOH to neutralize 150 mL of an HCl solution at an unknown concentration, what is the concentration of the HCl acid solution?
- The titration of 10.00 ml of an HCI solution of unknown concentration required 12.54 ml of 0.100 M NaOH solution to reach the equivalence point? What is the concentration of the unknown solution?
- The titration of 25.0 mL of an HCl solution of unknown concentration requires 45.3 mL of a 1.50 M NaOH solution to reach the equivalence point. What is the concentration of the unknown HCl solution?
- The titration of 10.00 mL of an HCl solution of unknown concentration requires 19.2 mL of a 0.400M NaOH solution to reach the equivalence point. What is the concentration of the unknown HCl solution?
- A 25.0 mL volume of HCl solution with an unknown concentration is titrated with a 0.208 M NaOH solution. Neutralization of the HCl solution requires 26.6 mL of the NaOH solution. Calculate the concentration of the HCl solution.
- A 25.0 mL volume of HCl solution with an unknown concentration is titrated with a 0.154 M NaOH solution. Neutralization of the HCl solution requires 22.6 mL of the NaOH solution. Calculate the concentration of the HCl solution.
- What volume (in mL) of 12 M HCI solution is required to prepare exactly 500 mL of a 0.12 M HCI solution?
- Water is added to 25.0 mL of a 0.750 M HCI solution until there is exactly 125 mL of solution. What is the concentration of the final solution?
- What is the molarity of an unknown HCI concentration if it requires 75 mL of a 0.2 M NaOH solution?
- 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?
- Suppose it requires 9.40 mL of a 0.10 M KOH solution to titrate 28.0 mL of an HCl solution of unknown concentration. Calculate the concentration of the HCl solution.
- 25.0 ml of HCl reacts with 39.5 ml of 0.150 M K3PO4 solution. 3HCl(aq) + K3PO4(aq) to H3PO4(aq) + 3KCl(aq). What is the concentration of the HCl solution? a) 0.0790 M b) 0.0949 M c) 0.237 M d) 0.711 M
- A 25.00 mL sample of HCl was titrated with 35.79 mL of 0.250 M KOH. Find the concentration of the HCl solution.
- 726 mL of 0.250 M HCl solution is mixed with 298 mL of 0.600 M HCl solution. What is the molarity of the resulting solution?
- A 50.0 ml sample of HCl is titrated until neutralized with exactly 25.0 ml of a 0.500 M NaOH solution. What was the concentration of the HCl?
- A solution of 0.0500 M HCI is used to titrate 28.0 mL of an ammonia solution of unknown concentration. The equivalence point is reached when 15.5 mL HCI solution have been added. (Assume K_w = 1.01 ti
- What is the molarity of an HCl solution if 5.3 mL HCl solution is titrated with 28.4 mL of 0.175? HCl(aq)+NaOH(aq) to NaCl(aq)
- Determine the molarity of an 18 ml sample of HCl solution that is required to prepare 30 ml of 2.3 M HCl solution.
- In standardizing a solution of HCl, it is found that 47.26 mL of the acid are equivalent to 1.216 g of pure Na_2CO_3, what is the normality of the acid?
- If 45 mL of 0.25 M HCl is required to completely neutralize 25.0 mL of NH3, what is the concentration of the NH3 solution?
- What is the concentration of each ion present in the solution formed by mixing 50 mL of 0.100 M HCl solution and 10.0 mL of 0.440 M HCl solution?
- What is the molarity of a solution that contains 8.25 g of Na2CO3 in 450 mL of solution?
- Find the Molarity We can measure the concentration of HCI solution by reaction with pure sodium carbonate: 2H^+ + Na_2CO_3 ? 2Na^+ + H_2O + CO_2. Complete reaction with 0.967 4 +/- 0.000 9 g of Na_2C
- In a titration, it is found that 97.7 mL of 0.154 M NaOH(aq) is needed to neutralize 25.0 mL of a solution of HCl(aq). Calculate the concentration of the HCl solution.
- What is the concentration of a HCl solution if 20.0 mL of the solution is neutralized by 15.0 mL of a 0.10 M Ca(OH)_2 solution? \\ A. 0.038 M B. 0.15 M C. 0.13 M D. 0.075 M
- What is the concentration of a HCl solution if 20.0 ml of the solution is neutralized by 15.0 ml of a 0.10 M Ca(OH)_2 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 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?
- In a titration of 50.0 ml of an HCl solution with an unknown concentration, 35.4 ml of a 0.504 M NaOH solution was required to reach the endpoint. What is the molarity M of the HCl solution?
- Na2CO3 + HCl titration Na2CO3 0,1 M 10 mL, HCl 0,1 M pH at V = 0 mL, 5 mL, 10 mL, 15 mL, 20 mL, 25 mL?
- By titration, it is found that 46.7 mL of 0.148 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the concentration of the HCl solution.
- By titration it is found that 42.9 mL of 0.163 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the concentration of the HCl solution.
- By titration, it is found that 73.5 mL of 0.158 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the concentration of the HCl solution.
- By titration it is found that 74.5 mL of 0.109 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the concentration of the HCl solution.
- By titration, it is found that 69.9 mL of 0.151 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the concentration of the HCl solution.
- By titration, it is found that 80.1 mL of 0.114 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the concentration of the HCl solution.
- By titration, it is found that 26.5 mL of 0.166 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the concentration of the HCl solution.
- Suppose you believe your unknown compound is Na_2CO_3, and you also prepare 20 mL of a 0.1 \dfrac{mol}{L} solution of it. Using a 0.2 \dfrac{mol}{L} HCl solution as the titrant, what volume of HCl (in mL) is needed to reach the equivalence point when me
- How many grams of Na_2CO_3 are required to completely react with 35.6 mL of a 0.315 M HCl solution? The reaction is: Na_2O_3(s) + 2HCl(aq) to 2NaCl (aq) + CO_2(g) + H_2O(I).
- A 20.0 ml sample of an unknown HCl solution requires titration with 15.0 ml of 0.1 M NaOH solution to reach equivalent point. What is the concentration of the HCl solution? The reaction is: HCl + NaOH
- A 25.0 ml aliquot of an HCl solution of unknown concentration is pipetted into a 125
- By titration, it is found that 76.7 mL of 0.130 M NaOH(aq) is needed to neutralize 25.0 mL of HCl (aq). Calculate the concentration of the HCl solution.
- 25.0 ml of 12.0 M HCl are diluted to 500 mL. What is the HCl concentration (molarity) of this dilute solution?
- What is the concentration of H+ in a 3.5 M HCI solution?
- What is the concentration of H+ in a 2.5 M HCI solution?
- What is the concentration of HCl when 25.0 mL of HCl completely reacts with 10.0 mL of 0.1 M solution of NH4OH?
- What is the concentration of a solution prepared by diluting 25.0 mL of HCL 0.750 mol/L to a final volume of 500 mL?
- Calculate the grams of Na2CO3 needed to react with 25.0 mL of 0.220 M HCl solution if one mole of Na2CO3 reacts with 2 moles of HCl.
- It requires 23.2 mL of 0.250 M KOH to titrate 49.0 mL of an HCl solution of unknown concentration. Calculate the initial HCl concentration.
- It requires 17.9 mL of 0.120 M KOH to titrate 78.0 mL of an HCl solution of unknown concentration. Calculate the initial HCl concentration.
- If 55 mL of 3.2 M HCl is used to make a 350 mL aqueous solution, what is the molarity of the dilute solution?
- What volume ml of a concentrated 6.0 m HCl solution is required to prepare 725 ml of .12 m HCl solution?
- If 45.0 mL of 0.25 M HCl is required to completely neutralize 25.0 mL of NH3, what is the concentration of the NH3 solution? HCl + NH3 to NH4Cl.
- 28 mL of 0.10 M HCl is added to 60 mL of 0.10 M Sr(OH)_2. Determine the concentration of OH^- in the resulting solution.
- A 20.0 mL sample of 0.875 M HCI solution was diluted to 150.0 mL. Calculate the molarity of the resultant solution.
- What mass of Na2CO3 (molar mass = 105.9887) can be neutralized with 25.00 mL of 3.11 M HCl?
- Calculate the volume of 4.000M HCl solution required to completely react with 1.700g of Na_{2}CO_{3}.
- What is the concentration when 54.0 mL of a 6.00 M HCl solution is diluted to 247 milliliters?
- You weigh out 0.966 g of an unknown sample and dissolve this in 50 mL of deionized water. Then, you titrate this solution with a standardized HCl solution whose concentration is 0.1125 M. 34.42 mL of the HCl titrant solution is required to reach the secon
- You add 3.5 L of an HCl solution of unknown concentration to 2.0 L of 0.5 M HCl and 4.5 L of water. The final concentration of HCl was 1.5 M. What was the unknown concentration of the initial HCl solution?
Explore our homework questions and answers library
Browse
by subject