Mixing copper sulfate and sodium hydroxide precipitates copper(II) hydroxide
the verdict
SUPPORTED
the evidence backs this
refutedsupported
the weight of evidence
6 sources for · 0 against
Peer-reviewed literature and reference materials confirm that combining copper(II) sulfate and sodium hydroxide results in a precipitation reaction yielding copper-containing hydroxide/oxide structures.
ABSTRACT The smelting reduction of spent lithium-ion batteries at high temperature results in metallic alloys containing cobalt, copper, nickel, and manganese, in addition to aluminum and lithium oxides. A process has been proposed to selectively recover high-purity powders of manganese dioxide, cobalt(II) sulfate, and nickel(II) sulfate from these metallic alloys. Initially, the metallic alloys were completely dissolved using a mixture of 2.0 M sulfuric acid and 15% (v/v) hydrogen peroxide with a pulp density of 25 g/L over a duration of 120 minutes. Subsequently, copper(II) ions were removed through cementation with manganese powder, and aluminum hydroxide was precipitated by adjusting the solution pH to 4.5 at room temperature. Pure manganese dioxide was then obtained from the resulting filtrate through oxidative precipitation, utilizing sodium hypochlorite as an oxidizing agent. The separation of cobalt(II) and nickel(II) was achieved via a two-stage counter-current extraction using a 20% saponified 0.5 M Cyanex 272 solution. The loaded cobalt(II) was stripped using a 0.3 M sulfuric acid solution, leading to the crystallization of cobalt(II) sulfate powders. The pH of the raffinate was adjusted to 9.0, resulting in the precipitation of nickel(II) hydroxide, which was subsequently dissolved to recover nickel(II) sulfate powders from the solution. Most of the experiments were conducted at ambient temperature, except for the evaporation stage of crystallization. Continuous experiments verified that the purity of the recovered cobalt, manganese, and nickel powders was 99.9%.
Copper(II) hydroxide chloride, Cu(OH)1.5Cl0.5, and copper(II) hydroxide nitrate, Cu(OH)1.5- (NO3)0.5, were precipitated by the stepwise addition of hydroxide to solutions containing Cu2+ at 10-4 or 10-3 M, and Cl - or NO3- at several concentrations between 10-3 and 10-1 M. The nature of the precipitates was confirmed by X-ray diffraction. pKs0 values estimated from the pH for 50% precipitation were 16.9 for Cu(OH)1.5Cl0.5 and 16.0 for Cu(OH)1.5(NO3)0.5. In each case, as OH- was added to a solution which contained Cu2+ with Cl - or NO3-, the pH rose initially to that characteristic of the formation of amorphous Cu(OH)2(pKs0 = 17.8), but decreased again after further additions of hydroxide or on aging to that characteristic of the more stable hydroxide chloride or hydroxide nitrate. It is suggested that Cu(OH)2 is an intermediate in the formation of Cu(OH)1.5Cl0.5 and Cu(OH)1.5(NO3)0.5.
hexaaquachromium(III)
Again, the precipitate is just the same as if you had added small amounts of either sodium hydroxide or ammonia solution. hexaaquairon(III)
. . . and again, exactly the same precipitate as if you had added any other base. Summary
In each case you get a precipitate of the neutral complex - the metal hydroxide. This is exactly the same precipitate that you get if you add small amounts of either sodium hydroxide solution or ammonia solution to solutions of these ions. Bubbles of carbon dioxide are also given off. 2+ ions
hexaaquacobalt(II)
No gas this time - just a precipitate of "cobalt(II) carbonate". hexaaquacopper(II)
Again, there isn't any carbon dioxide - just a precipitate of the "copper(II) carbonate". hexaaquairon(II)
You get a precipitate of the "iron(II) carbonate", but no carbon dioxide. Summary
Hexaaqua ions with a 2+ charge aren't sufficiently acidic to liberate carbon dioxide from carbonate ions. Instead you get a precipitate which you can think of as being the metal carbonate. Contributors and Attributions
- Jim Clark (Chemguide.co.uk)
An aqueous solution was prepared by mixing the copper(II) sulfate pentahydrate (CuSO 4 ), lactic acid, sodium hydroxide (NaOH) and de-ionized (DI) water. Direct deposition of copper(II) oxide (CuO) nanostructures films on glass substrates was achieved by a simple, inexpensive and one-step chemical bath deposition method. The pH of the solution was varied at 11.7, 12.0, 12.3 and 12.6 and immersed at low temperature (90 °C). The influences of the pH solution towards the surface topography, morphology and thickness were investigated by a field emission scanning electron microscopy (FESEM), an atomic force microscope (AFM) and a surface profiler. Meanwhile, an X-ray diffractometer (XRD) was used to examine the structural properties of CuO films. The optical properties were measured by a UV-Vis spectroscopy. It was found that the grain size of the films decreases and the surface becomes smoother and more uniform by increasing the pH solution. The CuO nanostructures have high crystallinity with monoclinic structure which is preferentially grown along ( ) and (200) directions. Therefore, the film has great potential for gas sensor device.
CuO is a well-known monoclinic structure with unique properties that is extensively investigated for sensor, energy storage, and optoelectronic applications. In this work, the CuO nanostructure was synthesized through facile precipitation by mixing the aqueous copper (II) sulfate pentahydrate with sodium hydroxide. The as-synthesized CuO was characterized by scanning electron microscopy (SEM), X-ray diffractometry (XRD), Fourier transform infrared spectroscopy (FTIR) and UV–visible spectroscopy. A homogeneous growth of a narrow, fine coral-like fibrous morphology was observed on CuO under SEM imaging. The FTIR spectra reveal the existence of some dominant sharp bands in the lower wavenumber region that represent the Cu-O bonds. The high solubility of CuO in water confirms the formation of particles with nanoscale dimensions. CuO exhibits a strong optical absorption peak at 510 nm, and the band gap determined by Tauc's relation is 2.11 eV. CuO is capable of inducing photocatalytic degradation on R6G dye solutions under low-intensity UVC irradiation, which can serve as a future photocatalyst for wastewater treatment.
Basic copper carbonate is a chemical compound, more properly called copper(II) carbonate hydroxide. It can be classified as a coordination polymer or a
Basic copper carbonate is a chemical compound, more properly called copper(II) carbonate hydroxide. It can be classified as a coordination polymer or a salt. It consists of copper(II) bonded to carbonate and hydroxide with formula Cu2(CO3)(OH)2. It is a green solid that occurs in nature as the mineral malachite. It has been used since antiquity as a pigment, and it is still used as such in artis
Basic copper carbonate is prepared by combining aqueous solutions of copper(II) sulfate and sodium carbonate. Basic copper carbonate precipitates from the solution, with release of carbon dioxide CO2:
2CuSO4 + 2Na2CO3 + H2O → Cu2(OH)2CO3 + 2Na2SO4 + CO2
Basic copper carbonate can also be prepared by treating aqueous solutions of copper(II) sulfate with sodium bicarbonate.
Copper(II) sulfate may also be substituted with Copper(II) chloride.
Everything we examined (6)
This check searched the claim as stated. It did not run a separate search for evidence against it.