Sodium bicarbonate reacts with dilute hydrochloric acid

\( \newcommand\) • • • • • • How They Work A modification of the extractions previously discussed in this chapter is to perform a chemical reaction in the separatory funnel in order to change the polarity and therefore partitioning of a compound in the aqueous and organic layers. A common method is to perform an acid-base reaction, which can convert some compounds from neutral to ionic forms (or vice versa). For example, imagine that a mixture of benzoic acid and cyclohexane is dissolved in an organic solvent like ethyl acetate in a separatory funnel. To separate the components, a water wash may be attempted to remove benzoic acid, but benzoic acid is not particularly water-soluble due to its nonpolar aromatic ring, and only small amounts would be extracted into the aqueous layer (Figure 4.54a). Figure 4.54: Washing a mixture of benzoic acid and cyclohexane with: a) water, b) aqueous \(\ce \left( aq \right)\) if desired to convert the benzoic acid back to its neutral form. Sodium Bicarbonate Washes An acid-base extraction can be used to extract carboxylic acids from the organic layer into the aqueous layer. As was discussed in the previous section, \(\ce\) could cause hydrolysis of the ester product. Extracting Bases Basic compounds such as amines can be extracted from organic solutions by shaking them with acidic solutions to convert them into more water-soluble salts. In this way, they can be extracted from an organic layer into an aqueous layer. \[\begin\] Extracting Ca...

acids and carbonates Chemguide: Core Chemistry 14 - 16 Reactions between acids and carbonates This page looks at the reactions between acids and carbonates to give a salt, carbon dioxide and water. A summary equation acid + carbonate salt + CO 2 + water Reactions involving calcium carbonate The commonest carbonate-acid reaction you will come across is that between calcium carbonate and dilute hydrochloric acid. Calcium carbonate occurs naturally as chalk, limestone and marble. The photo shows the reaction with marble chips. You get immediate fizzing with a colourless gas given off - that's carbon dioxide. The marble reacts to give a colourless solution of calcium chloride. CaCO 3(s) + 2HCl(aq) CaCl 2(aq) + CO 2(g) + H 2O(l) The reaction with dilute sulfuric acid is slightly more complicated because the calcium sulfate formed is only very slightly soluble. The reaction starts, but almost immediately stops again because the marble chips get coated with a layer of calcium sulfate which prevents any more acid getting at the marble chip. The photo shows what the reaction looks like a short time after you have added the acid. Nothing is happening. The ionic equation for the reaction All carbonates react in the same sort of way and that is because the same underlying bit of chemistry happens in each case. Carbonate ions from the carbonate react with hydrogen ions from the acid. CO 3 2-(s or aq) + 2H +(aq) CO 2(g) + H 2O(l) The "(s or aq)" is because a few carbonates (sodium, pota...

Sodium carbonate is more commonly known as washing soda. Like the similar-sounding compound sodium bicarbonate—baking soda—it's basic, and can react with acids. HCl, or hydrochloric acid, is a strong acid that reacts with sodium carbonate. The reaction produces large quantities of carbon dioxide gas, water and table salt. Sodium carbonate has the chemical formula Na2CO3. It has several different applications, one of which is producing certain kinds of glass. On a household level, however, sodium carbonate has everyday utility as a water softener. Many communities have large quantities of calcium and magnesium ions—positively charged particles—in the water, which prevent detergent from working as efficiently. Sodium carbonate added to water helps to remove magnesium and calcium ions, and increases detergent efficiency. HCl is the chemical formula for hydrochloric acid, which is a strong inorganic—meaning not carbon-based—acid, explains Dr. Martin Silberberg in his book "Chemistry: The Molecular Nature of Matter and Change." Like all acids, HCl has the ability to lose its hydrogen atom in water-based solution. If there's a base present, HCl gives its hydrogen to the base. This produces two new compounds, neither one of which is a strong acid or a strong base, and is called a neutralization reaction. When you mix sodium carbonate and HCl, two molecules of HCl give their hydrogen atoms to the sodium carbonate. This produces carbonic acid, with the formula H2CO3. The sodium fro...

Baking soda mainly contains sodium bicarbonate. When this is treated with dilute hydrochloric acid, the following reaction occurs. NaHCO3 + HCl → NaCl + CO2 + H2O Answer the questions below. i) What is the valency of the sodium ion? ii) What is the valency of the bicarbonate ion? iii) Is the chloride ion monovalent or divalent? iv) What do the symbols → and ↑ imply in the reaction? v) If one more H^ + ion is removed from bicarbonate ion gives carbonate ion. Write the formula of the carbonate radical. vi) The bicarbonate ion is anion.( Monoatomic / Polyatomic)vii) Name the products formed in the above reaction. viii) Identify the cation and the anion in the formula of Sodium chloride. ix) What is the difference between sodium and sodium ion. x) State the law which must be fulfilled, while balancing the chemical equation. Baking soda mainly contains sodium bicarbonate. When this is treated with dilute hydrochloric acid, the following reaction occurs. N a H C O 3 ​ + H C l → N a C l + C O 2 ​ + H 2 ​ O Answer the questions below. i) What is the valency of the sodium ion? ii) What is the valency of the bicarbonate ion? iii) Is the chloride ion monovalent or divalent? iv) What do the symbols → and ↑ imply in the reaction? v) If one more H + ion is removed from bicarbonate ion gives carbonate ion. Write the formula of the carbonate radical. vi) The bicarbonate ion is __________ anion.( Monoatomic / Polyatomic) vii) Name the products formed in the above reaction. viii) Identify t...

Sodium #color(darkblue)("bicarbonate")# #"Na"color(darkblue)("HCO"_3)# and hydrochloric acid #"HCl"# reacts to form sodium chloride, water, and carbon dioxide- an odorless gas- by the equation #"NaHCO"_3(aq)+"HCl"(aq) to "NaCl"(aq) + "H"_2"O"(l)+"CO"_2color(purple)((g))#. The mass of the system is not going to conserve if the reaction takes place in an open container: carbon dioxide escapes rapidly as the reaction proceeds, such that the mass of the products would be smaller than that of the reactants: #m("Reactants")=m("Products")# #color(white)(m("Reactants"))=m("Aqueous leftover")+m("CO"_2)# #m("Reactants") ge m("Aqueous leftover")# Verifying the conservation of mass for this reaction would, therefore, require trapping all gases produced within the system. A conical flask with an air-tight stopper is likely going to serve the purpose. Note, that given the fact that most electronic balances found in science labs are calibrated at room temperature and the exothermic nature of this reaction, it might be necessary to cool the system down to its initial temperature before taking any further measurements.