The impact of seawater with calcium and magnesium removal for the flotation of copper-molybdenum sulphide ores

The Influencing Mechanisms of Sodium Hexametaphosphate on Chalcopyrite Flotation in the Presence of MgCl2 and CaCl2

“…For instance, Nagaraj and Farinato [23] reported that reducing pH to a lower value can avoid the formation of precipitation, thereby increasing chalcopyrite flotation. However, the alkaline condition at pH 9~12 was used to depress pyrite that normally associated with chalcopyrite [24]. Therefore, it is impractical to reduce the pulp pH to neutral or acidity when using sea water in chalcopyrite flotation.…”

“…Therefore, it is impractical to reduce the pulp pH to neutral or acidity when using sea water in chalcopyrite flotation. Other researchers have attempted to add some reagents to achieve the goal [19,[24][25][26][27]. For instance, Jeldres et al [24] reported that the addition of CaO-Na 2 CO 3 mixtures can remove cations before flotation.…”

“…Other researchers have attempted to add some reagents to achieve the goal [19,[24][25][26][27]. For instance, Jeldres et al [24] reported that the addition of CaO-Na 2 CO 3 mixtures can remove cations before flotation. Hirajima et al [17] and Suyantara et al [28] found that emulsified kerosene was capable of reducing the adsorption of Mg(OH) 2 precipitation on chalcopyrite surface through forming kerosene and precipitation aggregates.…”

The Influence of Common Monovalent and Divalent Chlorides on Chalcopyrite Flotation

“…The presence of inorganic salts leads to more complex bubble coalescence, as inorganic ions-similar to frothers-can stabilize foams against coalescence and reduce bubble size [19,25]. The effects of salts on both floatability and frothability have been examined for copper ores [3,19,21,22,[26][27][28][29][30]. However, the effects of frothing characteristics of specific chloride salts on chalcopyrite flotation remain unclear.…”

An improved flotation test method and pyrite depression by an organic reagent during flotation in seawater

“…A high pH is commonly attained by lime addition, but the required amount is excessive due to the buffering effect of seawater, which increases the lime consumption by 5-10 times compared to fresh water (Castro, 2012;Veki, 2013). However, at pH values over 10.5, both calcium and magnesium ions form colloidal hydroxides, carbonates, and sulphates, which are detrimental for the recovery of molybdenite, and the quality of the concentrate is reduced (Castro and Laskowski, 2011;Ramos, Castro, and Laskowski, 2013;Jeldres et al, 2017). Some researchers have proposed that these complexes might precipitate onto the molybdenite surfaces and render them hydrophilic (Parraguez, Bernal, and Cartagena, 2009;Lucay et al, 2015).…”