Input interpretation
![HCl hydrogen chloride + NaHCO_3 sodium bicarbonate ⟶ NaCl sodium chloride + H_2CO_3 carbonic acid](../image_source/784795dd1907afa0d9e470603fb4b5b7.png)
HCl hydrogen chloride + NaHCO_3 sodium bicarbonate ⟶ NaCl sodium chloride + H_2CO_3 carbonic acid
Balanced equation
![Balance the chemical equation algebraically: HCl + NaHCO_3 ⟶ NaCl + H_2CO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 NaHCO_3 ⟶ c_3 NaCl + c_4 H_2CO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, C, Na and O: Cl: | c_1 = c_3 H: | c_1 + c_2 = 2 c_4 C: | c_2 = c_4 Na: | c_2 = c_3 O: | 3 c_2 = 3 c_4 Since the coefficients are relative quantities and underdetermined, choose a coefficient to set arbitrarily. To keep the coefficients small, the arbitrary value is ordinarily one. For instance, set c_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | HCl + NaHCO_3 ⟶ NaCl + H_2CO_3](../image_source/69133ab06f0de62c877f1e84d3621932.png)
Balance the chemical equation algebraically: HCl + NaHCO_3 ⟶ NaCl + H_2CO_3 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 HCl + c_2 NaHCO_3 ⟶ c_3 NaCl + c_4 H_2CO_3 Set the number of atoms in the reactants equal to the number of atoms in the products for Cl, H, C, Na and O: Cl: | c_1 = c_3 H: | c_1 + c_2 = 2 c_4 C: | c_2 = c_4 Na: | c_2 = c_3 O: | 3 c_2 = 3 c_4 Since the coefficients are relative quantities and underdetermined, choose a coefficient to set arbitrarily. To keep the coefficients small, the arbitrary value is ordinarily one. For instance, set c_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 1 c_3 = 1 c_4 = 1 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | HCl + NaHCO_3 ⟶ NaCl + H_2CO_3
Structures
![+ ⟶ +](../image_source/6d5c3f7e17749802a47d6ba3faeb6da1.png)
+ ⟶ +
Names
![hydrogen chloride + sodium bicarbonate ⟶ sodium chloride + carbonic acid](../image_source/3248515b578f02f05d5eb612ca62e209.png)
hydrogen chloride + sodium bicarbonate ⟶ sodium chloride + carbonic acid
Equilibrium constant
![Construct the equilibrium constant, K, expression for: HCl + NaHCO_3 ⟶ NaCl + H_2CO_3 Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the activity expression for each chemical species. • Use the activity expressions to build the equilibrium constant expression. Write the balanced chemical equation: HCl + NaHCO_3 ⟶ NaCl + H_2CO_3 Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i HCl | 1 | -1 NaHCO_3 | 1 | -1 NaCl | 1 | 1 H_2CO_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 1 | -1 | ([HCl])^(-1) NaHCO_3 | 1 | -1 | ([NaHCO3])^(-1) NaCl | 1 | 1 | [NaCl] H_2CO_3 | 1 | 1 | [H2CO3] The equilibrium constant symbol in the concentration basis is: K_c Mulitply the activity expressions to arrive at the K_c expression: Answer: | | K_c = ([HCl])^(-1) ([NaHCO3])^(-1) [NaCl] [H2CO3] = ([NaCl] [H2CO3])/([HCl] [NaHCO3])](../image_source/18c079bc83ebed134cccd9ea8ff2c479.png)
Construct the equilibrium constant, K, expression for: HCl + NaHCO_3 ⟶ NaCl + H_2CO_3 Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the activity expression for each chemical species. • Use the activity expressions to build the equilibrium constant expression. Write the balanced chemical equation: HCl + NaHCO_3 ⟶ NaCl + H_2CO_3 Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i HCl | 1 | -1 NaHCO_3 | 1 | -1 NaCl | 1 | 1 H_2CO_3 | 1 | 1 Assemble the activity expressions accounting for the state of matter and ν_i: chemical species | c_i | ν_i | activity expression HCl | 1 | -1 | ([HCl])^(-1) NaHCO_3 | 1 | -1 | ([NaHCO3])^(-1) NaCl | 1 | 1 | [NaCl] H_2CO_3 | 1 | 1 | [H2CO3] The equilibrium constant symbol in the concentration basis is: K_c Mulitply the activity expressions to arrive at the K_c expression: Answer: | | K_c = ([HCl])^(-1) ([NaHCO3])^(-1) [NaCl] [H2CO3] = ([NaCl] [H2CO3])/([HCl] [NaHCO3])
Rate of reaction
![Construct the rate of reaction expression for: HCl + NaHCO_3 ⟶ NaCl + H_2CO_3 Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the rate term for each chemical species. • Write the rate of reaction expression. Write the balanced chemical equation: HCl + NaHCO_3 ⟶ NaCl + H_2CO_3 Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i HCl | 1 | -1 NaHCO_3 | 1 | -1 NaCl | 1 | 1 H_2CO_3 | 1 | 1 The rate term for each chemical species, B_i, is 1/ν_i(Δ[B_i])/(Δt) where [B_i] is the amount concentration and t is time: chemical species | c_i | ν_i | rate term HCl | 1 | -1 | -(Δ[HCl])/(Δt) NaHCO_3 | 1 | -1 | -(Δ[NaHCO3])/(Δt) NaCl | 1 | 1 | (Δ[NaCl])/(Δt) H_2CO_3 | 1 | 1 | (Δ[H2CO3])/(Δt) (for infinitesimal rate of change, replace Δ with d) Set the rate terms equal to each other to arrive at the rate expression: Answer: | | rate = -(Δ[HCl])/(Δt) = -(Δ[NaHCO3])/(Δt) = (Δ[NaCl])/(Δt) = (Δ[H2CO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)](../image_source/6ceb79757a1beda4518f81f6760bf4f8.png)
Construct the rate of reaction expression for: HCl + NaHCO_3 ⟶ NaCl + H_2CO_3 Plan: • Balance the chemical equation. • Determine the stoichiometric numbers. • Assemble the rate term for each chemical species. • Write the rate of reaction expression. Write the balanced chemical equation: HCl + NaHCO_3 ⟶ NaCl + H_2CO_3 Assign stoichiometric numbers, ν_i, using the stoichiometric coefficients, c_i, from the balanced chemical equation in the following manner: ν_i = -c_i for reactants and ν_i = c_i for products: chemical species | c_i | ν_i HCl | 1 | -1 NaHCO_3 | 1 | -1 NaCl | 1 | 1 H_2CO_3 | 1 | 1 The rate term for each chemical species, B_i, is 1/ν_i(Δ[B_i])/(Δt) where [B_i] is the amount concentration and t is time: chemical species | c_i | ν_i | rate term HCl | 1 | -1 | -(Δ[HCl])/(Δt) NaHCO_3 | 1 | -1 | -(Δ[NaHCO3])/(Δt) NaCl | 1 | 1 | (Δ[NaCl])/(Δt) H_2CO_3 | 1 | 1 | (Δ[H2CO3])/(Δt) (for infinitesimal rate of change, replace Δ with d) Set the rate terms equal to each other to arrive at the rate expression: Answer: | | rate = -(Δ[HCl])/(Δt) = -(Δ[NaHCO3])/(Δt) = (Δ[NaCl])/(Δt) = (Δ[H2CO3])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)
Chemical names and formulas
![| hydrogen chloride | sodium bicarbonate | sodium chloride | carbonic acid formula | HCl | NaHCO_3 | NaCl | H_2CO_3 Hill formula | ClH | CHNaO_3 | ClNa | CH_2O_3 name | hydrogen chloride | sodium bicarbonate | sodium chloride | carbonic acid IUPAC name | hydrogen chloride | sodium hydrogen carbonate | sodium chloride | carbonic acid](../image_source/4244071bf90bfe1547ab33150517c65d.png)
| hydrogen chloride | sodium bicarbonate | sodium chloride | carbonic acid formula | HCl | NaHCO_3 | NaCl | H_2CO_3 Hill formula | ClH | CHNaO_3 | ClNa | CH_2O_3 name | hydrogen chloride | sodium bicarbonate | sodium chloride | carbonic acid IUPAC name | hydrogen chloride | sodium hydrogen carbonate | sodium chloride | carbonic acid
Substance properties
![| hydrogen chloride | sodium bicarbonate | sodium chloride | carbonic acid molar mass | 36.46 g/mol | 84.006 g/mol | 58.44 g/mol | 62.024 g/mol phase | gas (at STP) | solid (at STP) | solid (at STP) | melting point | -114.17 °C | 270 °C | 801 °C | boiling point | -85 °C | | 1413 °C | density | 0.00149 g/cm^3 (at 25 °C) | 2.16 g/cm^3 | 2.16 g/cm^3 | solubility in water | miscible | soluble | soluble | odor | | odorless | odorless |](../image_source/cb91cb8d296af38eea4da9f7e94fe5dc.png)
| hydrogen chloride | sodium bicarbonate | sodium chloride | carbonic acid molar mass | 36.46 g/mol | 84.006 g/mol | 58.44 g/mol | 62.024 g/mol phase | gas (at STP) | solid (at STP) | solid (at STP) | melting point | -114.17 °C | 270 °C | 801 °C | boiling point | -85 °C | | 1413 °C | density | 0.00149 g/cm^3 (at 25 °C) | 2.16 g/cm^3 | 2.16 g/cm^3 | solubility in water | miscible | soluble | soluble | odor | | odorless | odorless |
Units