Concentration of HCl can be measured by its reaction with Na2CO3: 2H+ + Na2CO3 –> 2Na+...

Concentration of HCl can be measured by its reaction with Na2CO3: 2H+ + Na2CO3 –> 2Na+ + H2O + CO2 A volume of 23.75 ± 0.04 mL HCL solution was required to completely react with 0.9674 ± 0.0009 g of Na2CO3. Given that FM of sodium carbonate is 105.988 ± 0.001 g. Find the molarity of HCl and its absolute uncertainty.

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queen_honey_blossom answered 1 year ago

The concentration of HCl can be determined by titration with a primary standard such as Na2CO3...

The concentration of HCl can be determined by titration with a primary standard such as Na2CO3 (sodium carbonate). The titration reaction isCO3^(2-) + 2H+ yields H2O + CO2What is the concentration of HCl if 25.9 mL of HCl was needed to to react with 0.311 g of Na2CO3 to reach the end point?

A solution of HNO3 is standardized by reaction with pure sodium carbonate. 2H^+ + Na2CO3 ------>...

A solution of HNO3 is standardized by reaction with pure sodium carbonate. 2H^+ + Na2CO3 ------> 2Na^+ + H2O + CO2 A volume of 28.28+-0.05 mL of HNO3 solution was required for complete reaction with 0.8711+-0.0007g of Na2CO3 (FM 105.988+-0.001). Find the molarity of the HNO3 and its absolute uncertainty with correct significant figures. [HNO3] = __________M +- __________ M Please help!!

A solution of HNO3 is standardized by reaction with pure sodium carbonate. 2H+ + Na2CO3 -->...

A solution of HNO3 is standardized by reaction with pure sodium carbonate. 2H+ + Na2CO3 --> 2Na+ + H2O + CO2 A volume of 27.87 ± 0.06 mL of HNO3 solution was required for complete reaction with 0.8538 ± 0.0008 g of Na2CO3, (FM 105.988 ± 0.001). Find the molarity of the HNO3 and its absolute uncertainty. Express the absolute uncertainty with three significant figures.

A solution of HNO3 is standardized by reaction with pure sodium carbonate. 2H+ + Na2Co3 arrowto...

A solution of HNO3 is standardized by reaction with pure sodium carbonate. 2H+ + Na2Co3 arrowto 2Na+ + H2O + CO2 A volume of 25.36+/- 0.06mL of HNO3 solution was required for complete reaction with 0.9572 +/- 0.0008 g of Na2CO3 (FM 105.988 +/- 0.001). Find the molarity of the HNO3 and its absolute uncertainty. HNO3= M +/- M (sig figs count for this) If you could show me step-by-step how to do this problem, that would be helpful.

For the reaction 2 HCl + Na2CO3 ----> 2 NaCl + H2O + CO2 8.0 moles...

For the reaction 2 HCl + Na2CO3 ----> 2 NaCl + H2O + CO2 8.0 moles of CO2 is collected at STP. What is the volume of CO2? 1.) 2.80 L 2.) 179 L 3.) 57.6 L 4.) 0.0250 L 5.) 22.4 L 6.) 0.357 L

Table A: Mass data for reaction of NaHCO3 - Na2CO3 mixture with HCl: Mass of crucible...

Table A: Mass data for reaction of NaHCO3 - Na2CO3 mixture with HCl: Mass of crucible and cover 33.2868 (g) Mass of crucible, cover, and mixture 33.7864 (g) Mass of crucible, cover, and residue after reaction with HCl (1st weighing) 33.7070 (g) Mass of crucible, cover, and residue after reaction with HCl (2nd weighing) 33.7012 (g) Mass of crucible, cover, and residue after reaction with HCl (3rd weighing) 33.7020 (g) Mass of unknown mixture used 0.4996 (g) Using the data...

Mass data for reaction of NaHCO3-Na2CO3 mixture with HCL Mass of crucible and cover (g) 28.8258...

Mass data for reaction of NaHCO3-Na2CO3 mixture with HCL Mass of crucible and cover (g) 28.8258 Mass of crucible, cover and mixture (g) 29.4948 Mass of crucible, cover and residue after reaction with HCL (g) 1st weighing... 29.4454 2nd weighing... 29.4455 Calculation of percent NaHCO3 and Na2CO3 in an unknown mixture. ( I need help filling out this chart) mass of unkown mixture used (g) mass of NaCl formed (g) Mass of NaHCO3 in unkown mixture (g) Mass of Na2CO3...

The concentration of HCl can be determined by titration with a primary standard such as sodium...

The concentration of HCl can be determined by titration with a primary standard such as sodium carbonate ( Na2CO3 ). The titration reaction is CO2−3+2H+⟶H2O+CO2 What is the concentration of HCl if 38.3 mL of HCl was needed to to react with 0.501 g of Na2CO3 to reach the end point?

Consider the reaction of sodium with carbon and ammonia. 2Na + 2C + 2NH3= 2NaCN +...

Consider the reaction of sodium with carbon and ammonia. 2Na + 2C + 2NH3= 2NaCN + 3H2 Determine the limiting reactant in a mixture containing 96.9 g of Na, 58.2 g of C, and 107 g of NH3. Calculate the maximum mass (in grams) of sodium cyanide, NaCN, that can be produced in the reaction.

Balance these equations: HCl+CaCO3= HCl+Na2CO3= HCl+NaOH= NaOH+FeCl3= CoCl2+AgNO3= CuSO4+Na2CO3= CuSO4+BaCl2= Na3PO4+CuSO4= Na3PO4+NiCl2= Na3PO4+BaCl2= NH4Cl+AgNO3=

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